CHEM 121 Lecture 17: 6.2 Concentration Based on Mass

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2 Nov 2017

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Concentration- the amount of solute dissolved in a given amount of solution. Concentration of a solution has an effect on. Physical properties (such as melting & boiling points) Amount of solute= mass of solute in grams (g) Concentration = amount of solute amount of solution. Concentration is expressed as a percentage by multiplying ratio by 100% Question 1: calculate the percent composition or % (m/v) of 2. 00 x 102 ml containing 20. 0 g sodium chloride. 2. 00 x 102 ml, total volume of solution. % (m/v) = 20. 0g nacl / 2. 00 x 102 ml x 100% = 10. 0% (m/v) sodium chloride. Question 2: calculate the number of grams of glucose in 7. 50 x 102 ml of a 15. 0% solution. Mass/mass percent: mass/mass percent is most useful for solutions of 2 solids whose masses are easily obtained, calculate % (mass/mass) of platinum in gold ring with 14. 00 g au and 4. 500g pt.

Related Questions

Solution concentrations are usually given as one of the following: â¢Mass percent (m/m)âthe mass of the solute in grams for exactly 100 g of solution â¢Volume percent (v/v)âthe volume of solute in exactly 100 mL of solution â¢Mass/volume percent (m/v)âthe mass of solute in grams for exactly 100 mL of solution â¢Molarity (M)âthe number of moles of solute in exactly 1 L of solution Calculate the mass percent (m/m) of a solution prepared by dissolving 59.86 g of NaCl in 160.1 g of H2O. Part B Vinegar is a solution of acetic acid in water. If a 285 mL bottle of distilled vinegar contains 24.4 mL of acetic acid, what is the volume percent (v/v) of the solution Part C Calculate the mass/volume percent (m/v) of 18.5 g NaCl in 64.5 mL of solution Part D Calculate the molarity (M) of 159.0 g of H2SO4 in 1.365 L of solution

1. The Solubity of nitrous oxide is 0.12g/100 g waterat 20 degrees celcius and 1.00 atm. What is the partial pressurerequired to dissolve 0.55 g of the gas in 100 g water at 20 degreescelcius?

2. Calcuate the mass/ mass percent concentration for: 2.50gK2Cr207 in 95.0g of solution

3. What mass of solution contains each of the following amountsof dissolved solutions? : 10.5g of acetic acid in 4.50%solution

4. How many grams of solute are dissolved in the followingsolutions?: 50.0 g of 5o.00% of Li2SO4 solution

5. What mass of water is necessary to prepare the solution,:100.0 g of 5.00% sugar solution

6. Calcuate the molar concentration for: 1.00g Na2CrO4 in 75.0mL of a solution

7. What volume of each of the following solutions contains theindicated amount of dissolved solute? 2.50g solute in 0.325 MAlBr3?

8. What is the mass of solution dissolved in the volume of 1.00L of 0.100M LiHCO3?

9. What is the molar concentration o a saturated solution ofcalcium hydroxide that contains 0.185 g solute in 1.00 mL ofsolution

10. Concentrated nitric acid is 16M. What is the volume of HNO3must be diluted with with distelled water to prepare 5.00L of 0.10M HNO3?

11. Given that 24.0mL of 0.170 M sodium iodide reacts with 0.209M mercury (II) nitrate solution according to this equation:

Hg(NO3)2+ NaI= HgI2+ NaNO3, so what is the mass of HgI2precipate?

1.This question has multiple parts. Work all the parts to get the most points.

In each of the following sets of ionic compounds, identify the members of the set that are soluble in water.

(Select all that apply.)

NH₄I

NH₄HCO₃

NH₄NO₂

NH₄NO₃

(Select all that apply.)

NaCH₃COO

AgCH₃COO

Cu(CH₃COO)₂

Cr(CH₃COO)₃

(Select all that apply.)

CaBr₂

Ca(OH)₂

CaSO₄

CaCl₂

(Select all that apply.)

Ca(NO₃)₂

CaSO₄

CaCO₃

Ca₃(PO₄)₂

2.Calculate the mass percent of solute in the following solutions.

(a) 8.94 g of NaCl dissolved in 55.5 g of H₂O	%
(b) 3.52 g of LiBr dissolved in 38.6 g of H₂O	%
(c) 14.4 g of KNO₃ dissolved in 260 g of H₂O	%
(d) 2.6Ã10^-3 g of NaOH dissolved in 3.8 g of H₂O	%

3.How many grams of water must be added to 49.5 g of NaOH in order to prepare a 6.73%(m/m) solution?

grams of water

4.Calculate the volume percent of 495 mL of acetone in enough water to give 1.07Ã10³ mL of solution.

%(v/v)

5.How many grams of Na₂CO₃ are needed to prepare 49.5 mL of a 4.27%(m/v) Na₂CO₃ solution?

grams of Na₂CO₃

6.For each of the following solutions, calculate the molarity of the solution.

9.87 g MgNH₄PO₄ in 750. mL solution

mol/L

19.1 g NaCH₃COO in 600. mL solution

mol/L

6.64 g CaC₂O₄ in 300. mL solution

mol/L

5.58 g (NH₄)₂SO₄ in 500. mL solution

mol/L

7.Calculate the number of grams of solute in each of the following solutions.

(a) 4.95 L of a 2.44 M HCl solution	grams of HCl
(b) 38.0 mL of a 12.5 M HNO₃ solution	grams of HNO₃
(c) 50.7 mL of a 10.4 M AgNO₃ solution	grams of AgNO₃
(d) 1.77 L of a 6.3Ã10^-3 M Na₂SO₄ solution	grams of Na₂SO₄

8.Calculate the mass-volume percent concentration for a 8.9 M NaOH solution.

9.What is the molarity of the solution prepared by diluting 35.0 mL of 1.25 M AgNO₃ to each of the following final volumes?

69.6 mL

84.9 mL

810 mL

2.57 L

CHEM 121 Lecture 17: 6.2 Concentration Based on Mass

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