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

Question

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

a

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

b

(Select all that apply.)

NaCH3COO

AgCH3COO

Cu(CH3COO)2

Cr(CH3COO)3

c

(Select all that apply.)

CaBr2

Ca(OH)2

CaSO4

CaCl2

d

(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) 2.6×10-3 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 1.07×103 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 6.3×10-3 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

M

84.9 mL

M

810 mL

M

2.57 L

a

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

b

(Select all that apply.)

NaCH3COO

AgCH3COO

Cu(CH3COO)2

Cr(CH3COO)3

Explanation / Answer

Too many questions, answering as much possible.

Normal rule of solubility: polar compounds are soluble in polar solvent. Water is polar. But there are plenty of exceptions and each exception has their own explanation.

1. a. all ammonium ions are soluble in water as they dissociate further to ammonia and proton.

b. All acetates are soluble except Ag-acetate because Ag+ ion is highly polarisable because of its large size. It forms strong bond with acetate that makes it insoluble.

c. All halides are soluble except some big cations like silver chloride. CaSO4 insoluble , Ca(OH)2 is slightly soluble(lime water). These are some exception from general rule.

d. Phosphates and carbonates are normally insoluble (except alkali metals). Only Ca(NO3)2 is soluble.

2. a Mass percent of solute in solution = 8.94/(8.94+ 55.5) * 100 % = 0.1387 * 100% = 13.87%

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