Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
pH vs. pOH

The pH and pOH of a compound helps to determine its acidity and basicity. 

The pH Scale

Concept #1: Understanding pH vs. pOH. 

pH stands for the negative logarithmic function of your hydronium concentration, whereas pOH stands for the negative logarithmic function of hydroxide concentration. 

Concept #2: The connection to Hydronium ion and Hydroxide ion concentrations. 

If we know the pH or pOH concentration then we can determine the concentration of hydronium ions or hydroxide ions. 

Concept #3: The pH Scale. 

If the pH is less than 7 then the solution is acidic, if the pH is equal to 7 then the solution is neutral and if the pH is greater than 7 then the solution is basic. 

Concept #4: The pH and pOH connection. 

Under normal conditions when the concentration is less than 1.0 M the pH scale is between 0 to 14. pH and pOH are connected by the following equation: 

Example #1: What is the hydroxide ion and hydronium ion concentration of an aqueous solution that has a pH equal to 6.12?

Practice: Which of the following solutions will have the lowest concentration of hydronium ions?

Practice: Which of the following statements about aqueous solutions is/are true?

Example #2: A solution is prepared by dissolving 0.235 mol Sr(OH)2 in water to produce a solution with a volume of 750 mL.

 

a) What is the [OH-]?

 

b) What is the [H+]?

Practice: What is the Kw of pure water at 20.0°C, if the pH is 7.083?

Auto – Ionization Product

Concept #5: Understanding the Auto-Ionization Reaction.

In a self-ionization reaction two water molecules react with one another, where one acts an acid and the other as a base. 

The ionization product of Kw is used in this self-ionization equation and ignoring solids and liquids gives the  equilibrium equation as: 

Example #3: Determine the concentration of hydronium ions for a neutral solution at 25oC and at 50oC.

pH of Strong Acids and Bases

If we have a STRONG ACID or STRONG BASE then we DO NOT use an ICE chart to find the pH of solution because the yield of H+ and OH  ions are known. 

Concept #6: Calculating the pH of a Strong Acid or Strong Base. 

Example #4: Calculate the pH of a 0.0782 M solution of CaH2.  

Example #5: Calculate the pH of a 0.000550 M HBr solution to the correct number of significant figures.

  1. 3.3
  2. 3.26
  3. 3.260
  4. 3.2596
  5. All are correct

Practice: Calculate the pH of 50.00 mL of 4.3 x 10-7 M H2SO4.

pH of Weak Acids and Bases

If we have a WEAK ACID or WEAK BASE then we DO use an ICE chart to find the pH of solution because the yield of H+ and OH  ions are unknown. 

Concept #7: Calculating the pH of a Weak Acid or Weak Base. 

To determine the pH of a weak acid or weak base we must use an ICE Chart. 

Example #6: Pryridine, an organic molecule, is a very common weak base.

 

C5H5N (aq) + H2O (l)  ⇌  C5H5NH+ (aq) + OH- (g)

 

Assume you have a 0.0225 M aqueous solution of pyridine, C5H5N, determine its pH. The Kb value for the compound is 1.5 x 10-9

Example #7: An unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 

Practice: Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 x 10-10.

Additional Problems
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A) 7.1 × 10-5 M B) 4.2 × 10-10 M C) 8.7 × 10-10 M D) 6.5 × 10-5 M E) 1.4 × 10-10 M
What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45? A) 2.82 × 10-11 M B) 3.55 × 10-4 M C) 3.45 M D) 10.55 M
What is the hydroxide ion and hydronium ion concentration of an aqueous solution that has a pOH equal to 6.29?
Calculate the pH of water at 40 oC, given that Kw is 3.8 x 10 -14 at this temperature. 
A solution with pH of 2 has twice the [H+] as as solution of pH 4. a. True b. False
A beaker contains a solution with [H3O+] = 2.59 x 10 -2 M at 25°C. Which of the following statement(s) is/are correct about this solution? i. The [OH-] in solution equal to 3.86 x 10 -6 M. ii. The pOH of the solutions is 12.41. iii. The beaker contains an acidic solution. A. i only B. ii only C. iii only D. i and ii E. ii and iii
What is the [OH -] for a solution at 25°C that has [H 3O+] = 2.35 x 10 -3 M? A) 4.26 x 10-5 M               B) 2.35 x 10-11 M                  C) 4.26 x 10-12 M D) 2.35 x 10-17 M              E) None of these choices is correct.
Calculate the pOH of a solution that contains 3.9 x 10 -4 M H3O+ at 25°C. A) 4.59 B) 3.31 C) 10.59 D) 9.14 E) 0.59
What is the [H3O+] for a solution at 25°C that has pOH = 5.640? A) 2.34 x 10-4 M B) 2.29 x 10-6 M C) 4.37 x 10-9 M D) 4.27 x 10-11 M E) 8.360 M
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C. A) 2.1 × 10-10 M B) 9.7 × 10-10 M C) 4.7 × 10-5 M D) 3.8 × 10-5 M E) 6.3 × 10-6 M
The pH of gastric juice inside the stomach is 1.5. What is [OH −]? Kw = 2.8 x10 -14 at body temperature (37 °C).
At 0 degrees Celsius, the ion product constant of water is 1.2x10-15. The pH of pure water at this temperature is:   A. 6.88 B. 7.00 C. 7.46 D. 7.56
What is the hydroxide concentration in a solution with a pH of 6.34?   A. 2.19x10-6 B. 2.19x10-8 C. 3.45x10-4 D. 3.45x10-6 E. 6.26x10-8
What is the hydronium ion concentration in a solution having a pOH of 3.62? 1. 3.8 × 10−5 M 2. 4.2 × 10−11 M 3. 3.8 × 10−4 M 4. 2.6 × 10−11 M 5. 5.1 × 10−10 M
For a solution that has a pH of 2.00, what is the concentration of OH  - ions? A. none present B. 0.0100 C. 1.00 x 10 −7 D. 1.00 x 10 −12 E. 1.00 x 10−16
What is the hydroxide ion and hydronium ion concentration of an aqueous solution that has a pH equal to 6.12?
If additional OH- is added to a sample of pure water, which of the following statements is incorrect?   a. The equilibrium position shifts to the left. b. The solution becomes more basic.  c. The [H3O+] remains unchanged. d. The [OH-] > [H3O+]. e. The amount of non-ionized H2O increases.  
What is the [H3O+] for a solution at 25°C that has pOH = 5.640? A) 2.34 x 10-4 M B) 2.29 x 10-6 M C) 4.37 x 10-9 M D) 4.27 x 10-11 M E) 8.360 M
Of the following, a solution with which pH would have the greatest concentration of hydronium ions? 1. 8  2. 9 3. 10 4. 12
Complete the following statement. A pH value of −1.5 1. indicates an H+ concentration of 31.6 M. 2. is impossible because pH cannot be negative. 3. indicates an H+ concentration of 0.0316M. 4. indicates an H+ concentration of −0.0176M. 5. indicates an H+ concentration of 0.176M. 6. indicates an H+ concentration of −0.0316M.
Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH.pH=2.00 M
Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH.pH=2.01 M
Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH.pH=2.02 M
Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic. pH pOH [H+] [OH-] Acidic or basic? 5.30 2.03 5.1×10−10 M 8.7×10−2 M Complete the first row of the table.
What happens to the [OH-] of a solution when the [H3O+] is increased? Decreased?
Define pH. What pH range is considered acidic? Basic? Neutral?
Is it possible for a solution to have a negative pH?
Define pOH. What pOH range is considered acidic? Basic? Neutral?
As the pH of a solution increases (gets higher), what happens to the acidity of the solution?
Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic. pH pOH [H+] [OH-] Acidic or basic? 5.30 2.03 5.1×10−10 M 8.7×10−2 M Complete the second row of the table.
Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic. pH pOH [H+] [OH-] Acidic or basic? 5.30 2.03 5.1×10−10 M 8.7×10−2 M Complete the fourth row of the table.
If the pOH for a solution is 3.00, what is the pH?
Consider two solutions, solution A and solution B. [H+] in solution A is 410 times greater than that in solution B.What is the difference in the pH values of the two solutions?
What is the [OH -] for a solution at 25°C that has [H 3O+ ] = 8.23 x 10 -2 M? A) ˃10-5 M B) 1.22 x 10-6 M C) 8.23 x 10-12 M D) 1.21 x 10-13 M E) 8.23 x 10-16 M
What is the concentration of hydroxide ions in pure water at 30.0°C, if K w at this temperature is 1.47 × 10-14? A) 1.00 × 10-7 M B) 1.30 × 10-7 M C) 1.47 × 10-7 M D) 8.93 × 10-8 M E) 1.21 × 10-7 M
Which answer is a true statement about pH values?a. A high pH value corresponds to a high H + concentration.b. Stomach acid has a high pH value.c. Pure water has a pH value of 0.d. pH is important in life mainly because it affects many everyday applications.e. None of the above.
What is the concentration (in M) of hydroxide ions (OH −) in a solution at 25.0 °C with pH = 4.282?      A) 9.72 B) 1.66 × 10 4 C) 1.91 × 10 −10 D) 5.22 × 10 −5 E) 4.28
pOH = 3.14 is equivalent to:       A) [OH −] = 3.14 × 10 −7 M B) pH = 11. C) [H +] = 1.4 × 10 −10 M D) [OH −] = 7.2 × 10 −4 M E) [H +] = 7.0 × 10 −4 M
Which is the pH of a solution with a [H  3O+] of 1 × 10 -9 M?a. -9.0b. 5.0c. -5.0d. 9.0e. None of the above 
If the concentration of hydronium ion, [H3O+] = 8.62 x 10 -4, what is the pH of the solution? a. 10.936 b. 0.998 c. 3.064 d.1.6 x 10-11 e. 2.329
Calculate the [H3O+] of a solution that has a pOH = 4.1.A. 1.3 x 10-10 MB. 9.9 MC. 7.9 x 109 MD. 2.4 x 10-15 ME. 4.1 x 10-11 M
For a solution with an [OH −] of 10−8 M, what would be the value of [H +] , pH and pOH, respectively? 1. 10−14 M, 6, 8 2. 10−6 M, 6, 8 3. 10−6 M, 8, 6 4. 106 M, 6, 8 5. 10−6 M, 6, 14 6. 10−14 M, 8, 6
Which statement correctly describes a solution with a pH of 9? a. It has a higher concentration of H 3O+ than OH - and causes litmus to turn blue. b. It has a higher concentration of OH - than H3O+ and causes litmus to turn blue. c. It has a higher concentration of H 3O+ than OH - and causes methyl orange to turn yellow. d. It has a higher concentration of OH - than H3O+ and causes methyl orange to turn red.
Which solution that has a pH of 2.00, what is the concentration of OH – ions?a. none presentb.0.0100c. 1.00 * 10–7d. 1.00 * 10–12e. 1.00 * 10–19
The lower the pH number, the higher is the hydrogen ion concentration.a. Trueb. False 
Which solution below has the highest concentration of hydroxide ions?a. pH= 3.21b. pH= 7.00c. pH= 7.93d. pH= 12.59e. pH= 9.82
Why is the pH of distilled water usually less than 7?
For the strong acid solution, determine [H 3O+], [OH-], and pH: 0.26M HCl 
In water, the equilibrium 2H2O(l) ⇌ H3O+ (aq) + OH−(aq)      Kc = 10−14 determines the concentrations of H3O+(aq) and OH -(aq). If the pH is 9.2, what is the OH - concentration? (note H3O+(aq) and H+(aq) are equivalent ways of representing a solvated proton and pH = -log[H+(aq)].) a) 9.76x10−6 b) 2.31x10−5 c) 3.88x10−4 d) 1.58x10−5 e) 2.54x10−6
Calculate [H3O+] and [OH−] for each of the following solutions. a. pH= 8.57  b. pH= 2.86
Complete the following table. All solutions are at 25°C. (Up to two significant figures)    
A solution is tested for pH and conductivity as pictured below:The solution contains one of the following substances: HCl, NaOH, NH4Cl, HCN, NH3, HF, or NaCN. If the solute concentration is about 1.0 M, what is the identity of the solute?
(b) What are [H3O+], [OH−], and pH in a solution with a pOH of 5.65?
(a) What are [H3O+], [OH−], and pOH in a solution with a pH of 8.97?
(b) What are [H3O+], [OH−], and pH in a solution with a pOH of 11.27?
Calculate [H +] and [OH -] for each solution at 25ºC. Identify each solution as neutral, acidic, or basic.b. pH = 15.3
Calculate [H +] and [OH -] for each solution at 25ºC. Identify each solution as neutral, acidic, or basic.c. pH = -1.0
Calculate [H +] and [OH -] for each solution at 25ºC. Identify each solution as neutral, acidic, or basic.d. pH = 3.20
How many moles of H3O+ or OH− must you add to a liter of strong acid solution to adjust its pH from 3.15 to 3.65 ?  Assume a negligible volume change.
Calculate [H +] and [OH -] for each solution at 25ºC. Identify each solution as neutral, acidic, or basic.e. pOH = 5.0
At 25°C, a saturated solution of benzoic acid (K a = 6.4 X 10 -5) has a pH of 2.80. Calculate the water solubility of benzoic acid in moles per liter.
How many moles of H3O+ or OH− must you add to a liter of strong base solution to adjust its pH from 9.33 to 9.07? Assume a negligible volume change.
Calculate [H +] and [OH -] for each solution at 25ºC. Identify each solution as neutral, acidic, or basic.f. pOH = 9.60
How many moles of H3O+ or OH− must you add to 5.6 L of strong acid solution to adjust its pH from 4.52 to 5.25? Assume a negligible volume change.
How many moles of H3O+ or OH− must you add to 87.5 mL of strong base solution to adjust its pH from 8.92 to 8.45? Assume a negligible volume change.
Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted rain to range from about 5.2 to 5.6.What is the range of [H+] in the raindrops?
The catalytic efficiency of an enzyme, called its activity, indicates the rate at which it catalyzes the reaction. Most enzymes have optimum activity over a relatively narrow pH range, which is related to the pH of the local cellular fluid. The pH profiles of three digestive enzymes are shown.Salivary amylase begins digestion of starches in the mouth and has optimum activity at a pH of 6.8; pepsin begins protein digestion in the stomach and has optimum activity at a pH of 2.0; and trypsin, released in pancreatic juices, continues protein digestion in the small intestine and has optimum activity at a pH of 9.5. Calculate [H3O+] in the local cellular fluid for each enzyme.
Human urine has a normal pH of 6.2. If a person eliminates an average of 1250 mL of urine per day, how many H+ ions are eliminated per week?
Calculate [H3O+] for a solution with a pH of 8.76.
Calculate the [OH -] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.a. [H+] = 1.0 x 10 -7 M
Calculate the [OH -] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.b. [H+] = 8.3 x 10 -16 M 
Calculate the [OH -] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.c. [H+] = 12 M
Calculate the [OH -] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.d. [H+] = 5.4 x 10 -5 M
Calculate the [H+] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.a. [OH -] = 1.5 M
Calculate the [H+] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.b. [OH -] = 3.6 x 10 -15 M
Calculate the [H+] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.c. [OH -] = 1.0 x 10 -7 M
Calculate the [H+] of each of the following solutions at 25ºC. Identify each solution as neutral, acidic, or basic.d. [OH -] = 7.3 x 10 -4 M
The molecular scene depicts the relative concentrations of H 3O+ (purple) and OH (green) in an aqueous solution at 25°C. (Counter ions and solvent molecules are omitted for clarity.) (b) How many H3O+ ions would you have to draw for every OH − ion to depict a solution of pH 4?
What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52?
Calculate the hydrogen ion concentration and the hydroxide ion concentration in wine from its pH. See following figure for useful information.
Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice from its pH. See following Figure for useful information.
The hydronium ion concentration in a sample of rainwater is found to be 1.7 X 10 −6 M at 25 °C. What is the concentration of hydroxide ions in the rainwater?
Environmental engineers use alkalinity as a measure of the capacity of carbonate buffering systems in water samples: Alkalinity (mol/L) = [HCO3−] + 2[CO32−] + [OH−] − [H+]Find the alkalinity of a water sample that has a pH of 9.5, 26.0 mg/L CO 32−, and 65.0 mg/L HCO3−.
The hydroxide ion concentration in household ammonia is 3.2 × 10 −3 M at 25 °C. What is the concentration of hydronium ions in the solution?
(a) What are [H3O+], [OH−], and pOH in a solution with a pH of 9.85?
(b) What are [H3O+], [OH−], and pH in a solution with a pOH of 9.43?
(a) What are [H3O+], [OH−], and pOH in a solution with a pH of 3.47?
(b) What are [H3O+], [OH−], and pH in a solution with a pOH of 4.33?
(a) What are [H3O+], [OH−], and pOH in a solution with a pH of 4.77?
Fill in the missing information in the following table.
Fill in the missing information in the following table.
The pH of a sample of gastric juice in a person’s stomach is 2.1. Calculate the pOH,    [H +], and [OH -] for this sample. Is gastric juice acidic or basic?
The pOH of a sample of baking soda dissolved in water is 5.74 at 25ºC. Calculate the pH, [H +], and [OH -] for this sample. Is the solution acidic or basic?
For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH.Express your answer using three significant figures. 8.74 × 10−3 M LiOHExpress your answer to three decimal places. [OH−],[H3O+] =Express your answer using three significant figures. 1.12 × 10−2 M Ba(OH)2Express your answer to three decimal places. [OH−],[H3O+] =Express your answer using three significant figures. 2.2 × 10−4 M KOHExpress your answer to three decimal places. [OH−],[H3O+] =Express your answer using three significant figures. 4.8 × 10−4 M Ca(OH)2Express your answer to three decimal places. [OH−],[H3O+] =
Arrange the following aqueous solutions, all at 25°C in order of decreasing acidity. a. pOH = 8.05 b. 0.0023M HCl c. pH= 5.45 d. 0.0018M KOH
Complete the table for each of the following solutions:
Calculate the pH and pOH of the solutions in the folowing:a. [H+] = 1.0 x 10 -7 M
Calculate the pH and pOH of the solutions in the folowing:b. [H+] = 8.3 x 10 -16 M 
Calculate the pH and pOH of the solutions in the folowing:c. [H+] = 12 M
Calculate the pH and pOH of the solutions in the folowing:d. [H+] = 5.4 x 10 -5 M
Calculate the pH and pOH of the solutions in the folowing:e. [OH -] = 1.5 M
Calculate the pH and pOH of the solutions in the folowing:f. [OH -] = 3.6 x 10 -15 M
Calculate the pH and pOH of the solutions in the folowing:g. [OH -] = 1.0 x 10 -7 M
Calculate the pH and pOH of the solutions in the folowing:h. [OH -] = 7.3 x 10 -4 M
If 1 mol of each of the following substances were dissolved in 1 L of water, which solution would contain the highest concentration of OH- ions?a. H2SO4b. NH4Clc. KNO3d. NaOH 
Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.
The binding of oxygen by hemoglobin in the blood involves the following equilibrium reaction: HbH+(aq) + O2(aq) ⇌ HbO2(aq) + H+(aq)In this equation, Hb is hemoglobin. The pH of normal human blood is highly controlled within a range of 7.35 to 7.45. Given the above equilibrium, why is this important? What would happen to the oxygen-carrying capacity of hemoglobin if blood became too acidic (a condition known as acidosis)?
The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid.You are told the liquid is pure water, a solution of HCl(aq), or a solution of KOH(aq). Which one is it?
For solution of the same concentration, as acid strength increas, indicate what happen to the following (increas, decreas, or doesn’t change).a. [H+]
The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid.Why is the temperature given on the pH meter?
For solution of the same concentration, as acid strength increas, indicate what happen to the following (increas, decreas, or doesn’t change).b. pH
For solution of the same concentration, as acid strength increas, indicate what happen to the following (increas, decreas, or doesn’t change).c. [OH-]
For solution of the same concentration, as acid strength increas, indicate what happen to the following (increas, decreas, or doesn’t change).d. pOH
Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2], known as TRIS, is a weak base used in biochemical experiments to make buffer solutions in the pH range of 7 to 9. A certain TRIS buffer has a pH of 8.10 at 25°C and a pH of 7.80 at 37°C. Why does the pH change with temperature?
The two molecular scenes shown depict the relative concentrations of H 3O+ (purple) in solutions of the same volume (with counter ions and solvent molecules omitted for clarity). If the pH in scene A is 4.8, what is the pH in scene B?
What is the pH of pure water at 40C if the kw at this temperature is 2.92x10-14?
Calculate the pH of each acid solution.[H3O+] = 0.041 M
Calculate the pH of each acid solution.[H3O+] = 0.042 M
Calculate the pH of each acid solution.[H3O+] = 0.043 M
Classify the solutions as acidic or basic.a. [OH–] = 1.1 x 10–9 Mb. [OH–] = 2.9 x 10–2 Mc. [OH–] = 6.9 x 10–12 M
Calculate the pH of each solution and indicate whether the solution is acidic or basic.[H3O+] = 1.5 x 10-4
A site in Pennsylvania receives a total annual deposition of 2.688 g/m 2 of sulfate from fertilizer and acid rain. The mass ratio of ammonium sulfate/ammonium bisulfate/sulfuric acid is 3.0/5.5/1.0. (c) If 10. km2 is the area of an unpolluted lake 3 m deep and there is no loss of acid, what pH will the lake water attain by the end of the year? (Assume constant volume.)
The molecular scene depicts the relative concentrations of H3O+ (purple) and OH (green) in an aqueous solution at 25°C. (Counter ions and solvent molecules are omitted for clarity.) (a) Calculate the pH.
Calculate [OH-] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. A solution in which [H+] is 1000 times greater than [OH-]. Express your answer using two significant figures.[OH-] = _____ M
What is the pH of a .025 M HCl solution?
What is the pH of a solution that has a [H +] = 0.0045 M? a. 2.35 b. None of these c. 1.35 d. 7.0045 e. 3.35
Calculate the pH of a solution at 25°C in which the [OH−] = 5.4 x10  −7 M.A) 4.51B) 7.05C) 7.73D) 6.38E) 8.40
At 0°C the ion product constant of water,  Kw, is 1.2 x 10–15. The pH of pure water at this temperature is(A) 6.88(B) 7.00(C) 7.46(D) 7.56
A patient with respiratory alkalosis has a blood plasma pH of 7.59. What is the [H3O+] of the blood plasma? Express your answer to two significant figures and include the appropriate units.
At body temperature of 37.0°C, K w = 2.5 x 10-14. Calculate the [H3O+] if the [OH -] = 3.9 x 10-3 M.A. 2.5 x 10-12 MB. 6.4 x 10-12 MC. 3.9 x 10-3 MD. 1.0 x 10-7 ME. 2.5 x 10-14 M
A change in pH of 1.0 unit indicates that: 1. the volume of H+ in a solution changes by an order of magnitude.2. the acid or base content decreases or increases by 0.1 M.3. the molarity of H+ changes by one order of magnitude.4. the acid or base content decreases or increases by 1.0 M.5. the salt content decreases or increases by 1.0 M.
Complete this table of values for four aqueous solutions at 25°C.
Trimethylamine, (CH3)3N, is a weak base (Kb = 6.4 × 10–5) that hydrolyzes by the followingequilibrium: (CH3)3N + H2O → (CH3)3NH+ + OH– What is the pH of a 0.1 M solution of (CH 3)3NH+? (Enter pH to 2 decimal places; hundredth's.)
What is the pH of an aqueous solution with the hydronium ion concentration [H  3O+] = 2 x 10 -14 M ?
Calculate the [H3O+] and pH of each of the following H 2SO4 solutions.a) Calculate the [H3O+] for 0.10 M solution. Express your answer using two significant figures. b) Calculate pH for 0.10 M solution. Express your answer using two decimal places.
Which of the following solutions is basic?i. [H3O+] = 2 x 10 -8 Mii. [OH-] = 2 x 10 -6 Miii. [H3O+] = 9 x 10 -6 Ma. i , ii, and iiib. iiic. iid. i and ii
The pH values of five solutions are given below. Which is the most alkaline?a. pH = 4.5b. pH = 13.0c. pH = 0.0d. pH = 1.0e. pH = 7.0
In an acidic solution, how does the concentration of hydronium ions compare to the concentration of hydroxide ions?a) Hydronium ion is greater than hydroxide ion.b) There is not enough information to tell.c) They are equal.d) Hydronium ion is less than hydroxide ion.
Complete this table of values for four aqueous solutions at 25°c 
An aqueous solution at 25°C has a H3O+ concentration of 0.0076 M. Calculate the OH- concentration. Be sure your answer has the correct number of significant digits.
What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 12.3?
Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic.pHpOH[H+][OH-]Acidic or basic?5.302.035.1×10−10 M8.7×10−2 MComplete the third row of the table.
 Calculate the poH of a 0.0321 M HCIO4 solution at the following temperatures
Calculate either [H3O+] or [OH -] for the solutions below at 25°C. a) [OH-] = 1.21 x 10-7 M     [H3O+] =  b) [H3O+] = 8.05 x 10-9 M     [OH-] =c) [H3O+] = 0.000589 M    [OH-] =Which of these solutions are basic at 25°C? a)         b)         c)
What is the pH of a neutral solution at a temperature where Kw = 9.9 times 10-14? Express your answer numerically using two decimal places.
What are the concentrations of OH- and H+ in a 0.00052 M solution of Ba(OH)2 at 25°C? Assume complete dissociation. [OH-] = [H+] =
Calculate either [H3O+] or [OH-] for the solutions below. a) [OH-] = 3.21 x 10-7 M b) [H3O+] = 9.73 x 10-9 M c) [H3O+] = 0.000551 M Which of these solutions are basic at 25°C?
Calculate the H3O+ concentration for each pH: a) pH = 13b) pH = 2 c) pH = 8 
Calculate [H3O+] for the following solutions:a) 6.00 x 10-3 M HBrb) 1.80 x10-2 M KOH
(a) What is the pH of 3.7 times 10^-3 M HCI? (b) What is the pH of 8 times 10^-8 M HCI?
0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to this solution? Express the pH numerically to two decimal places. pH = 11.75 What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places.
1. Three solutions have the following pH:      pH = 4.3      pH = 6.8      pH = 11.5      a) Which solution contains the highest H3O+ ion concentration?     b) Which solution is the most acidic?     c) Which solution is the most basic?2. What is the difference between a strong acid and a weak acid?3. Calculate [H3O+] and [OH-] for the following three solutions      a) pH = 9.5      b) pH = 3.6      c) pH = 7.0
At 25 C, how many dissociated OH ions are there in 1219 mL of an aqueous solution whose pH is 1.56? 
Complete this table of values for three aqueous solutions at 25 c.
What is the concentration of OH - in a 0.1 M solution of HI? 1 x 10-12 M 0.1 M 1 x 10-13 M 0.00001 M
Calculate either [H3O+] or [OH -] for the solution below. Which of these solutions are basic at 25°C?
What is the pH of an aqueous solution with a hydrogen ion concentration of [H+] = 7.3 times 10-9 M?
Calculate the pH of the following aqueous solutions at 25°C, K w at 25°C is 1.01e-14. (a) 3.2 x 10-11 M KOH ___________ (b) 7.6 x 10-7 M HNO3 _________
Calculate the concentrations of H 3O+ and OH− in each of the following solutions:i) Human blood (pH 7.40)ii) A cola beverage (pH 2.8)
Calculate the pH and the pOH of an aqueous solution that is 0.040 M in HCl(aq) and 0.055 M in HBr(aq) at 25°C.
Calculate the pOH of a 0.0448 M HCIO4 solution at the following temperatures. a) 5°Cb) 45°C
Part AIf the [H3O+] is 4.950 x 10-12, what is the pH? (i) -11.305 (ii) 11.3 (iii) 2.020 x 10-12 (d) 11.305
Calculate the hydronium ion, H3O+, and hydroxide ion, OH-, concentrations for a 0.0244 M HCI solution. [H3O+] = [OH-] = 
Complete this table of values for three aqueous solutions at 25°C.
Calculate the pH of an aqueous solution that is 0.020 M in HCl (aq) at 25°C.  
Determine the concentration of H+ in the following solutions at 25°C: a) a solution with pH = 2.0 [H+] =  b) a solution  [H+] =  c) a solution with pOH = 10.0 [H+] = 
Complete this table of values for three aqueous solutions at 25°C.
What is the pH of a 3.0 M solution of HCIO4?
What are [H3O+], [OH-], and pOH in a solution with a pH of 3.22? 
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definition of pH is in terms of base 10 logarithms. pH = - log [H +] where [H+] is the hydrogen ion concentration. (A) If the hydrogen ion concentration in a solution is 1.36 x 10 -3 mol/L the pH is __________. (B) If the pH of a solution is 4.108, the hydrogen ion concentration is _________ mol/L.
Calculate [H+], and [OH-] in an aqueous solution that is 0.115 M in HCLO 4(aq) at 25°C. Is the solution acidic, basic or neutral? 
Calculate [OH-] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. [H+] = 6.5 x 10-10 M. Express your answer using two significant figures.
Given that KN for water is 2.4 x 10-14 M2 at 37 °C, Compute the pH of a neutral aqueous solution at 37 °C, which is the normal human body temperature.Is a pH = 7.00 solution acidic, basic, or neutral at 37 °C? 
Question 2Calculate the pH of a solution with [OH-] equal to 2.9 x 10-4 M. 
A solution has a pH of 3 and another has a pH of 7. What is true? (a) The pH 3 has more Hydrogen ions than the pH7 and is an acid. (b) The pH 7 is neutral and has more H+ ions than the pH3. (c) pH 3 is a base and pH 7 is neutral
The question has multiple parts. Work on all the parts to get the most points.Determine the [H+] value for solutions with the following characteristics: a. pH = 9.59 b. pH = 2.40 c. pH = 5.39 
Calculate the pH of a 0.03 M solution of Ca(OH)2. Select one: a. 1.48 b. 12.52 c. 1.18 d. 12.82 e. None of these
Calculate the pH of a 0.0477 M KOH solution at the following temperatures.a) 10°Cb) 50°C
Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is the molar concentration of H3O+ in a cola that has a pH of 4.240? Express your answer with the appropriate units. Rank the following from most to least acidic. Rank from most to least acidic. To rank items as equivalent, overlap them.[H3O+] = 10-2               [H3O+] = 10-6            pH = 14          pH = 3                pH = 5
Calculate the pH of each of the following strong acid solutions. Part A8.90 x 10-3 M HNO3. Express your answer using three decimal places.Part B0.600 g of HClO4 in 2.90 L of solution. Express your answer using three decimal places. 
A solution of NaOH(aq) contains 6.6 g of NaOH(s) per 100.0 mL of solution. Calculate the pH and the pOH of the solution at 25°C. pH = pOH = 
Calculate [H3O+] given [OH -] in each aqueous solution.  Express your answer using two significant figures. Part A[OH -] = 6.1 x 10 -11 M Part BClassify this solution as acidic or basic. Part C[OH -] = 7.0 x 10 -9 M 
Calculate pH for each H3O+ concentration: a) [H3O+] = 1 x 10 -6 M b) [H3O+] = 0.001 M c) [H3O+] = 1 x 10 -12 M
The hydronium ion concentration of an aqueous solution of 0.348 M formic acid, HCOOH (Ka = 1.80 x 10-4) is 
[OH-] = 5.5 x 10-9 M Express the molarity to two significant figures. 
A patient with respiratory alkalosis has a blood plasma pH of 7.58. What is the [OH  -] of the blood plasma? Express your answer to two significant figures and include the appropriate units.
Calculate the pH and the pOH of an aqueous solution that is 0.050 M in HCl(aq) and 0.060 M in HBr(aq) at 25°C.
Calculate the pH of each of the following strong acid solutions. Part C5.00 mL of 1.50 M HCl diluted to 0.530 L. Express your answer using three decimal places. Part DA mixture formed by adding 45.0 mL of 2.5 x 10-2 M HCl to 150 mL of 1.5 x 10-2 M HI. Express your answer using two decimal places. 
You have a solution with a hydronium ion concentration of 1.0 times 10 -7 M. What is the hydroxide ion concentration in this beaker? a. 0.01 Mb. 1 x 10-12 Mc. 12 M d. 2 Me. 1 x 10-7 Mf. 1 x 10-10 M  
What are the H3O+ and OH- concentrations of solutions that have the following pH values? Part ApH3 Express your answer using one significant figure separated by a comma.
What are the concentrations of H 3O+ and OH- in oranges that have a pH of 3.76? 
Be sure to answer all parts.What are [H3O+], [OH -], and pOH in a solution with a pH of 11.50? 
What is the concentration of OH- and pOH in a 0.00058 M solution of Ba(OH)2 at 25°. Assume complete dissociation. [OH-] =pOH =  
Calculate the pH of a 0.0279 M HCl solution. Your answer should be to the nearest tenth.
Calculate [H3O+] for the following solutions:a. 3.44 x 10-3 M HBr[H3O+] = b. 1.50 x 10-2 M KOH[H3O+] =  
Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. Part A[OH-] = 5.5 x 10-4 M. Express your answer using two significant figures. Part B                       • the solution is acidic                       • the solution is basic                        • the solution is neutral    
Calculate the [OH-] of peas with the [H3O+] = 5.5 times 10-7 M
Which of these statements are true for a neutral, aqueous solution at 25 degree C? More than one can be correct. a. pH = 7.00b. pOH = 7.00c. [H+] = [OH -]Which of these statements are true for a neutral, aqueous solution regardless of temperature? More than one can be correct. a. pH = 7.00b. pOH = 7.00c. [H+] = [OH -]