General Chemistry

Practice

1.

Provide a balanced chemical equation for the dissociation of each compound:

 

a) Na3PO4,  b) K2CrO4,  c) MgCl2,  d) Al(NO3)3,  e) HNO3,  f) K2SO4,  g) Ca(NO2)2,  h) Mg(C2H3O2)2,  i) Na2CO3,  j) (NH4)2SO4,  k) HClO4,  l) NaHSO3, 

a)
answer
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b)
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c)
answer
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d)
answer
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e)
answer
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f)
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g)
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h)
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i)
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j)
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k)
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l)
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2.

Write balanced complete ionic and net ionic equations for each reaction:

 

a) K2SO4(aq) + CaCl2(aq) →CaSO4(s) + 2KCl(aq)

b) Na2S(aq) + 2HBr(aq) → 2NaBr(aq) + H2S(g)

c) NH4Cl(aq) + KOH(aq) → KaCl(aq) + H2O(l) + NH3(g)

d) Na2CO3(s) + H2SO4(aq) → Na2SO4(aq) + CO2(g)+ H2O(l)

e) AgNO3(aq) + NaI(aq) → Agl(s) + NaNO3(aq)

f) HBr(aq) + KOH(aq) → KBr(aq) + H2O(l)

g) HC2H3O2(aq) + Na2CO3(aq) → NaC2H3O2(aq) + CO2(g) + H2O(l)

h) LiOH(aq) + HC2H3O2(aq) → LiC2H3O2(aq) + H2O(l)

i) HCl(aq) + NH3(aq) → NH4Cl(aq)

j) 2K3PO4(aq) + 3BaCl2(aq) → Ba3(PO4)2(s) + 6KCl(aq)

a)
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b)
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c)
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d)
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e)
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f)
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g)
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h)
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i)
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j)
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3.

Complete and balance each of the following molecular equations in aqueous solution:

 

a) AgNO3(aq) + CaCl2(aq) →

b) HNO3(aq) + Na2CO3(aq) →

c) K2CO3(s) + HClO3(aq) →

d) Al(OH)3(s) + HBr(aq) →

e) H3PO4(aq) + Fe(OH)3(s) →

f) BaCl2(aq) + K2SO4(aq) →

a)
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b)
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c)
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d)
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e)
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f)
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4.

Calculate the molarity of each ion in the following solutions:

 

a) 0.150 M NaNO3
b) 0.250 M K2SO4
c) 0.280 M Ca(NO3)2
d) 0.350 M AlCl3

a)
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b)
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c)
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d)
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5.

Which solution contains more chloride ions assuming complete solubility of salts?

 

a) 0.140 M NaCl or 0.060 M AlCl3
b) 0.250 M BaCl2 or 0.250 M MgCl2
c) 0.250 M MgCl2 or 0.450 M KCl

a)
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b)
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c)
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6.

How many ml of 1.80 M MgBr2 is necessary to precipitate all the silver ions in 600.0 mL of 0.80 M AgNO3 solution?

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7.

How many ml of 2.70 M K2SO4 is required to precipitate all the barium ions in 500. mL of 0.650 M BaCl2 solution?

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8.

27.0 mL of a NaOH solution was needed to neutralize 0.326 g of KHP (KHC8H4O4). What is the molarity of the NaOH solution?

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9.

What volume of 0.150 M calcium hydroxide is required to neutralize 250.0 mL of 0.0350 M sulfuric acid?

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10.

How many mL of 0.250 M HCl will neutralize 60.00 mL of 0.060 M Ba(OH)2?

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11.

What is the mass in grams of AgCl precipitate if 20.0 mL of 0.150 M AgNO3 is added to 45.0 mL of 0.250 M MgCl2?

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12.

How many mL of 0.600 M K2SO4 was added to 400.0 mL of 0.500 M BaCl2 solution if 31.2 g of precipitate was collected?

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13.

When a 42.0-mL sample of a 0.85 M sodium chloride solution is mixed with 17.0 mL of a 0.650 M lead(II) nitrate solution, 2.45 g of a precipitate is formed:

2NaCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2NaNO3(aq)

What are the theoretical and the percent yields of the reaction?

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14.

A 4.598-g sample of acetylsalicylic acid (the active ingredient in aspirin) was dissolved in water. It took 35.6 mL of a 0.717 M NaOH solution to neutralize the acid. Determine the molar mass of the acid considering that it is a monoprotic acid.

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15.

A student prepared a solution by dissolving 2.40-g mixture of calcium nitrate and calcium chloride. To this, a solution of silver nitrate was added dropwise until the mass of the precipitate stayed constant at 0.584 g. Determine the mass percent of calcium nitrate in the mixture.

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16.

Determine the products and calculate the mass of the precipitate that is formed after 177.2 mL of a 1.25 M Na2CrO4(aq) solution is mixed with 250 mL of a 1.25 M AgNO3(aq) solution.

AgNO3(aq) + Na2CrO4(aq) →

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