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,
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)
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) →
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
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
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?
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?
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?
What volume of 0.150 M calcium hydroxide is required to neutralize 250.0 mL of 0.0350 M sulfuric acid?
How many mL of 0.250 M HCl will neutralize 60.00 mL of 0.060 M Ba(OH)2?
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?
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?
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?
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.
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.