Subjects

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Molarity | 23 mins | 0 completed | Learn Summary |

Normality & Equivalent Weight | 24 mins | 0 completed | Learn Summary |

Solution Stoichiometry | 22 mins | 0 completed | Learn |

Solubility Rules | 7 mins | 0 completed | Learn Summary |

Net Ionic Equations | 21 mins | 0 completed | Learn Summary |

Electrolytes | 19 mins | 0 completed | Learn Summary |

Redox Reaction | 32 mins | 0 completed | Learn Summary |

Balancing Redox Reactions | 22 mins | 0 completed | Learn |

Activity Series | 19 mins | 0 completed | Learn |

End of Chapter 4 Problems | 46 mins | 0 completed | Learn |

Additional Practice |
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Redox Reactions |

Calculate Oxidation Number |

Additional Guides |
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Dilution |

Net Ionic Equation |

Oxidation Reduction (Redox) Reactions |

Oxidation Number |

Types of Chemical Reactions |

In this video we take a look at the concept of dilutions and the equations associated with dilutions. Any time we are talking about dilutions we use the equation of M₁V₁ = M₂V₂.

M₁ here represents the molarity or concentration before dilution has occurred

V₁ represents the volume before dilution has occurred

M₂ represents the molarity or concentration after dilution

V₂ represents your volume after dilution

Some key things in relation to the variables to one another:

M₁ represents your concentration before dilution. It is more concentrated because we haven’t added water yet. Therefore, M₁ is always a larger value than M₂, it is a larger molarity.

V₂, since that’s the volume after we’ve added water, V₂ will be larger than M₁. Since V₂ represents our final volume after we’ve added water, V₂ equals V₁ plus the amount of water you’ve added. That’s the whole process of dilution, adding water.

In terms of dilution, they’ll refer to two molarities or two volumes for a single compound.

For example, you have 50 ml of 0.100 M NaOH and you are going to dilute it so that you get to a new concentration of 0.012 M NaOH. Realize that we are talking about only one compound the whole time and they have given us two molarities. That’s the key to realizing dilution is occurring - referring to one compound and that one compound is either dealing with two molarities or two volumes right from the beginning of the question.

Now, they also could mention or reference as “mixing or adding water to the solution” which represents a dilution and it’s a signal to you that the dilution formula will most likely be used to answer the question.

Remember, when we talk about dilutions it is just simply adding water to a reaction mixture. It causes our solution to become less concentrated so your M₂ is smaller than your M₁. Because you are adding water, the overall volume increases that’s why your V₂ (your final volume) is bigger than V₁ (your initial volume).

How many milliliters of a 0.266 M LiNO 3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution?
A) 42.3 mL
B) 35.1 mL
C) 23.6 mL
D) 53.2 mL
E) 18.8 mL

What volume (in mL) of 0.0887 M MgF 2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution?
A) 72.3 mL
B) 91.8 mL
C) 14.4 mL
D) 69.4 mL
E) 10.9 mL

To what volume should you dilute 1.25 L of a 5.00 M SrBr 2 solution to obtain a 0.500 M SrBr2 solution?
A. 1.25 L
B. 12.5 L
C. 5.00 L
D. 0.450 L

If you take 59.0 ml of a 0.75 M solution of NaBr and dilute it to 900 ml, what will the molarity of the final solution be?

What volume of 12 M HCl solution is required to prepare exactly 500.0 mL of a 0.60 HCl solution?
(A) 10 mL
(B) 14 mL
(C) 25 mL
(D) 40 mL

A solution of 0.512 M KOH is diluted from 1.32 L to 2.4 L. What is the final concentration of KOH?

To what final volume would 100 mL of 5.0 M KCl have to be diluted in order to make a solution that is 0.54 M KCl?

A student prepared a stock solution by dissolving 25.00 g of NaOH in enough water to make 150.0 mL of solution. The student then took 20.0 mL of the stock solution and diluted it with enough water to make 250.0 mL of a solution. The student then took 75.0 mL of this solution and dissolved in water to make a 500 mL solution. What is the concentration of NaOH for this final solution? (MW of NaOH: 40.00 g/mol).
a. 2.20 M
b. 0.0495 M
c. 0.0347 M
d. 0.0145 M

Calculate the molarity of acetate ions from a solution prepared by diluting 52.7 mL of 0.250 M tin (IV) acetate to 250 mL.
a. 0.2108 M C2H3C2-
b. 0.0527M C2H3C2-
c. 1.1850 M C2H3C2-
d. 0.1054 M C2H3C2-

How many milliliters of a 9.0 M H 2SO4 solution are needed to make 0.35 L of a 3.5 M solution?

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL.
a) 0.0887 M
b) 0.0313 M
c) 0.0199 M
d) 0.0501 M
e) 1.13 M

If you take 59.0 mL of a 0.75 M solution of NaBr and dilute it to 900 mL, what will the molarity of the final solutions be?

A chemist has a 3.50 M NaOH solution. If they add 25.00 mL of this solution to a 500 mL volumetric flask and fill it up to the line with water, what is the concentration of the final solution?
a) It is still 3.50 M
b) 0.175 M
c) 0.0875 M
d) 0.35 M
e) 0.00875 M

If you take 10.0 mL of concentrated NH 3 which has a molarity of 14.8 M and dilute it to 0.500 L, what will be the concentration of the final diluted solution?
a) 1.48 M
b) 1.00 M
c) 0.148 M
d) 0.296 M
e) 14.8 M

Determine the concentration of NO3− ions in a solution prepared by diluting 25.0 mL of a 0.188 M Sr(NO3)2 stock solution to 0.150 L. 1L = 1000 mL
A) 31.3 M
B) 0.0887 M
C) 0.0313 M
D) 0.0199 M
E) 0.0627 M

If 125 mL of water is added to 225 mL of 0.254 M NaCl, what is the final concentration (in M) of NaCl? Assume volumes are additive, and enter your answer with 3 decimal places and no units.

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL.
A) 1.13 M
B) 0.0501 M
C) 0.0887 M
D) 0.0199 M
E) 0.0313 M

Solution A is composed of a 2.00 M aqueous solution of NaCl. Solution B is composed of a 1.25 M aqueous solution of NaCl. Which is the more dilute solution?
A. Solution A
B. Solution B

Calculate the following quantity: Volume of 2.050 M copper (II) nitrate that must be diluted with water to prepare 750.0mL of a 0.8553 M solution.

A student wants to prepare 250 mL of 0.10 M NaCl solution. Which procedure is most appropriate?
Formula Molar Mass of NaCl is 58.4 g•mol –1.
a) Add 5.84 g of NaCl to 250 mL of H 2O.
b) Add 1.46 g of NaCl to 250 mL of H 2O.
c) Dissolve 5.84 g of NaCl in 50 mL of H 2O and dilute to 250 mL.
d) Dissolve 1.46 g of NaCl in 50 mL of H 2O and dilute to 250 mL.

What volume, in liters, of 6.11 M NaOH solution would you need to prepare 580.0 mL of a 0. 135 M NaOH solution by dilution? (molar mass NaOH = 40.00 g/mole)

How many milliliters of a 0.266 M LiNO 3 solution are required to make a 150.0 mL of 0.075 M LiNO3 solution?
a) 18.8 mL
b) 35.1 mL
c) 42.3 mL
d) 23.6 mL
e) 53.2 mL

The image below represents a small volume within
550
mL
of aqueous ethanol (CH3CH2OH) solution. (The water molecules have been omitted for clarity.)
Which image below best represents the same volume of the solution after we add an additional
550
mL
of water?

If you dilute 16.0 mL of the stock solution to a final volume of 0.310 L , what will be the concentration of the diluted solution?

If 124 mL of a 1.2 M glucose solution is diluted to 550.0 mL , what is the molarity of the diluted solution?

If 4.0 L of a 4.9 M
SrCl2 solution is diluted to 50 L , what is the molarity of the diluted solution?

To what volume should you dilute 50.5 mL of a 5.05 M
KI solution so that 25.5 mL of the diluted solution contains 3.30 g of KI?

How many milliliters of a stock solution of 6.20
M
HNO3 would you have to use to prepare 0.160 L of 0.510
M
HNO3?

What is the concentration of HCl in the final solution when 65 mL of a 9.0 M HCl solution is diluted with pure water to a total volume of 0.15 L?

How much water should you add to 40.5 mL of a 2.65 M iron (III) chloride, FeCl 3, stock solution to make a 1.50 M solution?
A) 71.6 mL
B) 31.1 mL
C) 22.9 mL
D) 17.6 mL
E) 10.2 mL

What volume of a 2.00 M KCl solution is required to prepare 500 mL of a 0.100 M KCl solution?

What is the molarity of sodium ions in a solution prepared by diluting 250 mL of 0.550 M Na2SO4 to 1.25 L?a) 0.110 Mb) 0.138 Mc) 0.220 Md) 0.275 M

How many milliliters of water would be needed in order to dilute 75.0 mL of 0.50 M NaOH to 0.020 M?

Patrick Star took 33.0 mL of a 1.50 M solution of KI and diluted it to 400.0 mL. What was the resulting molarity of his solution? a) 8.08b) 1.32 x 104c) 7.58 x 10-5d) 18.18e) 0.124

When making up a solution of accurately known volume, one has to allow the solution to reach room temperature before bringing the volume up to the mark because: a) the same mass of a liquid will occupy different volumes at different temperaturesb) heat may be evolved when a liquid is added to a solid in a flaskc) heat may be evolved when two liquids are added together in a flaskd) none of the above is truee) all of the above is true

If 25.00 mL of 1.50 M HCl(aq) is diluted with water to a volume of 750.0 mL, what is the molarity of the diluted HCl(aq)?a. 2.22 x 10-2 Mb. 5.00 x 10-2 Mc. 2.07 x 10-3 Md. 4.50 x 101 Me. 1.35 x 103 M

If 880 mL of water is added to 125.0 mL of a 0.770 M HBrO 4 solution, what is the resulting molarity? a. 0.674 Mb. 0.109 Mc. 0.630 Md. 0.096 M

A 230.-mL sample of a 0.275 MCaCl 2 solution is left on a hot plate overnight; the following morning, the solution is 1.10 M. What volume of water evaporated from the 0.275 M CaCl2 solution?

(a) How many milliliters of a stock solution of 10.0 M HNO 3 would you have to use to prepare 0.450 L of 0.500 M HNO3?

(b) If you dilute 25.0 mL of the stock solution to a final volume of 0.500 L, what will be the concentration of the diluted solution?

To prepare 100.0 mL of a 0.100 M copper(II) chloride solution from 0.500 M copper(II) chloride, pipet into a volumetric flask(A) 10.0 mL of the 0.500 M solution and then add water until the total volume is 100.0 mL.(B) 20.0 mL of the 0.500 M solution and then add water until the total volume is 100.0 mL.(C) 20.0 mL of the 0.500 M solution into 80.0 mL of water.(D) 40.0 mL of the 0.500 M solution into 60.0 mL of water.

Concentrated HCl has a density of 1.19 g/mL and is 38.0% by mass HCl (the rest of the mass is water). How many mL of this concentrated solution do you need to add to a 250.0 mL volumetric flask to create a 0.0500 M HCl solution? Give your answer to the hundredths decimal place and do not include any units. The MW of HCl is 36.46 g/mol.

Equal volumes of a 6.0 M KNO3 solution and 2.6 M NaCl solution are mixed. What is the molarity of the new solution in KNO3 and NaCl?
a. 6.0 M KNO3 and 2.6 M NaCl
b. 2.6 M KNO3 and 6.0 M NaCl
c. 12.0 M KNO3 and 5.2 M NaCl
d. 3.0 M KNO3 and 1.3 M NaCl
e. none of the above

How many milliliters of a 0.266 M LiNO 3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution?
A) 42.3 mL
B) 35.1 mL
C) 23.6 mL
D) 53.2 mL
E) 18.8 mL

What volume (in mL) of 0.0887 M MgF 2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution?
A) 72.3 mL
B) 91.8 mL
C) 14.4 mL
D) 69.4 mL
E) 10.9 mL

Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 25 mL of the concentrated HCl, adding it to water, and diluting to 0.800 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density.

If 30.0 mL of water is added to 50.0 mL of a 6.00 M solution. What will be the new concentration of the solution?

How many mL of water should be added to 375 mL of a 0.250 M solution of HCl in order to dilute it to a 0.080 M solution?

To what volume should you dilute 60.0 mL of a 8.0 M HNO 3 solution to obtain a 0.100 M solution?

A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00-mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

A solution is prepared by dissolving 0.5842 g oxalic acid (H 2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the oxalic acid solution?

To what final volume should you dilute 0.50 L of a 0.05 M aqueous sugar solution to obtain a 0.03 M sugar solution? How much water (L) did we add?

Calculate each of the following quantities:Molarity of a solution prepared by diluting 37.00 mL of 0.250 M potassium chloride to 150.00 mL

Calculate each of the following quantities:Molarity of a solution prepared by diluting 25.71 mL of 0.0706 M ammonium sulfate to 500.00 mL

Explain what changes and what stays the same when 1.00 L of a solution of NaCl is diluted to 1.80 L

The figures below are molecular-level representations of four aqueous solutions of the same solute. Arrange the solutions from most to least concentrated.

Calculate the molarity of the following aqueous solutions.30.0 mL of 3.60 M HNO3 diluted to 0.250 L

If 4.12 L of a 0.850 M-H3PO4 solution is be diluted to a volume of 10.00 L, what is the concentration of the resulting solution?

What is the concentration of the NaCl solution that results when 0.150 L of a 0.556-M solution is allowed to evaporate until the volume is reduced to 0.105 L?

What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume? (a) 1.00 L of a 0.250-M solution of Fe(NO3)3 is diluted to a final volume of 2.00 L

What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?(b) 0.5000 L of a 0.1222-M solution of C3H7OH is diluted to a final volume of 1.250 L

What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?(c) 2.35 L of a 0.350-M solution of H3PO4 is diluted to a final volume of 4.00 L

What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?(d) 22.50 mL of a 0.025-M solution of C12H22O11 is diluted to 100.0 mL

What is the final concentration of the solution produced when 225.5 mL of a 0.09988-M solution of Na2CO3 is allowed to evaporate until the solution volume is reduced to 45.00 mL?

Calculate the molarity of each aqueous solution: (a) 78.0 mL of 0.240 M NaOH diluted to 0.250 L with water

Calculate the molarity of each aqueous solution:(b) 38.5 mL of 1.2 M HNO3 diluted to 0.130 L with water

If you take a 13.0-mL portion of the stock solution and dilute it to a total volume of 0.550 L , what will be the concentration of the final solution?

A solution is prepared by dissolving 0.6706 g oxalic acid (H 2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the oxalic acid solution?

Describe how you would prepare 2.00 L of 0.250 M NaOH from 1.00 M NaOH stock solution.

Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from 1.75 M K2CrO4 stock solution.

How would you prepare 1.00 L of a 0.50-M solution of H 2SO4 from “concentrated” (18 M) sulfuric acid?

How would you prepare 1.00 L of a 0.50-M solution of HCl from “concentrated” (12 M) reagent?

How would you prepare 1.00 L of a 0.50-M solution of HNO 3 from “concentrated” (16 M) reagent?

A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00-mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.

A standard solution is prepared for the analysis of fluoxymesterone (C 20H29FO3), an anabolic steroid. A stock solution is first prepared by dissolving 10.0 mg of fluoxymesterone in enough water to give a total volume of 500.0 mL. A 100.0-mL aliquot (portion) of this solution is diluted to a final volume of 100.0 mL. Calculate the concentration of the final solution in terms of molarity.

A stock solution containing Mn 2+ ions was prepared by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution:For solution A, 50.00 mL of stock solution was diluted to 1000.0 mL.For solution B, 10.00 mL of solution A was diluted to 250.0 mL.For solution C, 10.00 mL of solution B was diluted to 500.0 mL.Calculate the concentrations of the stock solution and solutions A, B, and C.

Calculate each of the following quantities:Volume (L) of 1.63 M calcium chloride that must be diluted with water to prepare 350. mL of a 2.86×10−2 M chloride ion solution

Calculate each of the following quantities:Final volume (L) of a 0.0700 M solution prepared by diluting 18.0 mL of 0.155 M lithium carbonate with water

What volume of a 1.50 M HCl solution should you use to prepare 2.00 L of a 0.100 M HCl solution?

What volume of a 1.00-M Fe(NO3)3 solution can be diluted to prepare 1.00 L of a solution with a concentration of 0.250 M?

An experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many mL of 11.9 M HCl would be required to make 250 mL of 2.00 M HCl?

What volume of a 1.00 M stock solution of glucose must be used to make 500.0 mL of a 1.75 X 10-2 M glucose solution in water?

Describe how you would prepare each of the following aqueous solutions.Give the volume of the solute and volume of the solvent for a 0.50 M solution of HCl that would just neutralize 6.0 g of Ba(OH)2 starting with 6.0 M HCl.

You have a stock solution of 15.2 M NH3. How many milliliters of this solution should you dilute to make 1300 mL of 0.260 M NH3?

To what volume (in milliliters) should you dilute 100.0 mL of a 4.50 M solution of CaCl2 solution to obtain a 0.800 M solution of CaCl2?

What volume of a 5.10 M solution of NaNO3 do you need to make 0.505 L of a 1.40 M solution of NaNO3?

To what volume should you dilute 51 mL of a 13 M stock HNO3 solution to obtain a 0.126 M HNO3 solution?

To what volume should you dilute 30 mL of a 12 M H2 SO4 solution to obtain a 0.16 M H2 SO4 solution?

Muriatic acid, an industrial grade of concentrated HCl, is used to clean masonry and cement. Its concentration is 11.7 M.Write instructions for diluting the concentrated acid to make 3.0 gallons of 3.5 M acid for routine use (1 gal = 4 qt; 1 qt = 0.946 L).

A 230.-mL sample of a 0.275-M CaCl2 solution is left on a hot plate overnight; the following morning, the solution is 1.10 M. What volume of water evaporated from the 0.275 M CaCl2 solution?

Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M KCl solution to 250.0 mL. A) 0.0160 M B) 0.00800 M C) 0.340 M D) 0.0320 M E) 2.50 M

The circle below represents 1.0 liter of a solution with a solute
concentration of 1 M:Explain what you would add (the amount of solute or volume of solvent) to the solution so as to obtain a solution represented by each of the figures (a) - (c)?

What volume (L) of a 1.5 M KOH solution can be prepared by diluting 0.2 L of a 5M KOH solution? Show your work.

How is the molarity of a 0.50 M KBr solution changed when water is added to double its volume?

To what volume (in mL) must a 3.45 M lead(II) nitrate solution be diluted in order to make 450.0 mL of a 0.990 M solution of lead(II) nitrate?A. 129B. 109C. 101D. 56.0E. 45.0

How many mL of 3.0M H2SO4 are required to make 1.5L of 0.10M H2SO4?a) 0.020mL b) 20.mL c) 0.050mL d) 50.mL e) 33mL

What is the molarity of each of the following solutions?40.0 mL of 9.00 M H2 SO4 diluted to 0.500 L

What is the concentration of a solution made by diluting 35 mL of 6.0 M HCI to a final volume of 750 mL?

Calculate the concentration of an oxalic acid (H 2C2O4) solution when 73.4 mL of water is added to 31.5 mL of a 3.03 M oxalic acid solution?A. 10.1 MB. 1.30 MC. 0.910 MD. 2.12 ME. 2.28 M

A 0.200 M K2SO4 solution is produced by ____.A) dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 LB) dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mLC) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mLD) dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mLE) dilution of 1.00 mL of 250 M K2SO4 to 1.00 L

What volume (L) of 0.18 M H2SO4 can be prepared by diluting 143 mL of 5.5 M H2SO4 ?

Your lab partner messes up and accidentally makes the needed solution of NaCl too concentrated, 150.0 mL of a 0.78 M solution, when you needed 150.0 mL of a 0.45 M solution. You sigh, and add water to dilute the solution. What is the final volume of your corrected 0.45 M NaCl solution?A. 86.5 mLB. 1,730 mLC. 260. mLD. 520. mL E. 192 mL

How many liters of 0.750 M NH3(aq) do you need to make a 0.50 L of 0.250 M NH3(aq) solution?A. 0.167 B. 0.177 C. 0.681 D. 0.125 E. 0.560

How many milliliters of a 9.0 M H 2SO4 solution are needed to make 0.45 L of a 3.5 M solution?

Write a detailed set of instructions for making two solutions: (1) 100 mL of 16 MNaOH from solid sodium hydroxide and (2) 1.00 L of 0.1 M NaOH from your first solution. You have in your lab: volumetric flasks marked to contain 100.0 mL and 1.000 L,
a graduated cylinder, and a balance.Calculate the volume (in mL) of 16 M NaOH solution needed to make a 1.00 L solution of 0.1 M NaOH.

If 0.1718 L of a 0.3556-M C3H7OH solution is diluted to a concentration of 0.1222 M, what is the volume of the resulting solution?

How many milliliters of 11.5 M HCI(aq) are needed to prepare 765.0 mL of 1.00 M HCl(aq)?

What volume of a 0.33-M C12H22O11 solution can be diluted to prepare 25 mL of a solution with a concentration of 0.025 M?

A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

What is the concentration of H^+ ions in a solution of hydrochloric acid that was prepared by diluting 30.0 mL of concentrated (11.6 M) HCl to a final volume of 500 mL?

It is desired to prepare 0.500 L of a 0.17l M solution of NaCl from a 1.00 M stock solution. How many mL of the stock solution must be taken for the dilution? Enter your answer in the provided box.

To what volume should you dilute 20 mL of a 11 M stock HCl solution to obtain a 0.500 M HCl solution? Express your answer using two significant figures.

How much of a 15.0 M HNO3 solution should you use to make 830.0 mL of a 0.250 M HNO3 solution?

To what volume should you dilute 35 mL of a 11 M stock HCl solution to obtain a 0.600 M HCl solution?

How much 12.0 M HCl stock solution in mL must be used to prepare 268 mL of 0.561 HCl?

70.0 mL of a 1.30 M solution is diluted to a total volume of 238 mL. A 119-mL portion of that solution is diluted by adding 125 mL of water. What is the final concentration? Assume the volumes are additive.

A puddle of coastal seawater, caught in a depression formed by some coastal rocks at high tide, begins to evaporate on a hot summer day as the tide goes out. If the volume of the puddle decreases to 29% of its initial volume, what is the concentration of Na+ after evaporation if initially it was 0.449 M?

Part BWhat is the final volume in millilitres when 0.731 L of a 45.0 % (m/v) solution is diluted to 23.4 % (m/v)? Express your answer with the appropriate units.Part C A 506 mL NaCl solution is diluted to a volume of 1.06 L and a concentration of 7.00 M. What mi the initial concentrate? Express your answer with the appropriate units.

If the volume of the puddle decreases to 25.0 % of its initial volume, what is the concentration of Na+ after evaporation if initially, it was 0.449 M?

What volume of 3.00 M SrCl 2 is needed to prepare 525 mL of 5.00 mM SrCl 2?

What is the concentration of a solution made by diluting 35 mL of 6.0 M HCI to a final volume of 750 ml?

A puddle of coastal seawater, caught in a depression formed by some coastal rocks at high tide, begins to evaporate on a hot summer day as the tide goes out. If the volume of the puddle decreases to 26% of its initial volume, what is the concentration of Na+ after evaporation if initially it was 0.449 M?

65.0 mL of a 1.70 M solution is diluted to a total volume of 208 mL. A 104-mL portion of that solution is diluted by adding 189 ml of water. What is the final concentration? Assume the volumes are additive.

You have 47.0 mL of a 0.400 M stock solution that must be diluted to 0.100 M. Assuming the volumes are additive, how much water (mL) should you add?

63.0 mL of a 1.20 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 109 mL of water. What is the final concentration? Assume the volumes are additive.

Calculate the concentration of a solution made by diluting 88.0 mL of 6.0 M HBr to a final volume of 625.0 mL.

A 4.15 M sugar solution is diluted from 120.0 mL to 850.0 mL. What is the concentration of the dilute solution?

Hydrochloric acid is usually purchased in a concentrated form hat is 370% HCl by mass and has a density of 1.20 g/mL.Part AHow much concentrated solution would you take to prepare 3.05 L of 0.440 M HCI by mixing with water?

51.0 mL of a 1.50 M solution is diluted to a total volume of 268 mL. A 134-mL portion of that solution is diluted by adding 149 mL of water. What is the final concentration? Assume the volumes are additive.

You wish to make a 0.190 M hydroiodic acid solution from a stock solution of 6.00 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution?

In the laboratory, a student dilutes 20.5 mL of a 7.01 M hydrobromic acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution?

How many milliliters of 11.5 M HCI(aq) are needed to prepare 320.0 mL of 1.00 M HCI(aq)?

72.0 mL of a 1.20 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 177 mL of water. What is the final concentration? Assume the volumes are additive.

63.0 mL of a 1.30 M solution is diluted to a total volume of 268 mL. A 134 mL portion of that solution is diluted by adding 117 mL of water. What is the final concentration? Assume the volumes are additive.

In the laboratory you dilute 5.39 mL of a concentrated 12.0 M hydroiodic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution?

You have 97.0 mL of a 0.500 M stock solution that must be diluted to 0.100 M. Assuming the volumes are additive, how much water should you add?

A student needs to prepare 50.0 mL of 1.00 M aqueous H2O2 solution. Calculate the volume (mL) of 5.0 M H2O2 stock solution that should be used.

A 14.0 M solution of concentrated nitric acid has 20.0 mL withdrawn from it. The 20.0 mL sample is then diluted until the total volume of the resulting solution is 2.50L. What is the concentration of the dilute solution?a. 0.593 Mb. 0.280 Mc. 0.112 Md. 0.094 Me. 0.045 M

In the laboratory you dilute 5.00 mL of a concentrated 12.0 M hydroiodic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution?

You wish to make a 0.257 M hydrobromic acid solution from a stock solution of 6.00 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution?

A beaker contains 100 grams of 0.60 M NaCI. If you transfer 50 grams of the solution to another beaker, what is the molarity of the solution remaining in the first beaker?

What volume of 0.750 M NH3(aq), in L, would you use to prepare 0.500 L of 0.250 M NH3(aq) solution?

What volume of a 4.20 M solution of NaNO3 do you need to make 0.460 L of a 1.60 M solution of NaNO3? Express the volume to three significant figures and include the appropriate units.

A 5.0 - L sample of a 6.3 M NaCl solution is diluted to 70 L. What is the molarity of the diluted solution? Express your answer using two significant figures.

Calculate each of the following quantities:Molarity of sodium ion in a solution made by mixing 3.58 mL of 0.348 M sodium chloride with 500. mL of 6.81×10−2 M sodium sulfate (assume volumes are additive)

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