Question

# 1) sulfuric acid reacts with the ammonia according to the equation below. It takes 32.89 mL...

1) sulfuric acid reacts with the ammonia according to the equation below. It takes 32.89 mL of a 1.50 M solution of sulfuric acid to neutralize 64.7 mL of ammonia solution. what is the molar concentrationof the ammonia solution? H2SO4 (aq) + 2 NH3 (aq)---> (NH4)2SO4 (aq)

2) A 500.0mL solution that contains silver ion is treated with excess sodium chloride soultion, producing a precpitate of silver chloride that has a mass of 45.4 mg. What mass of silver ion was present in the original 500.0 mL sample (give the mass in mg)? Ag+ (aq) + Cl- (aq) --> AgCl (s)

H2SO4 (aq) + 2 NH3 (aq)---> (NH4)2SO4 (aq)

1mole H2SO4=2mole NH3

M1V1/n1 = M2V2/n2

Conc.of H2SO4 =M1= 1.50M, V1=32.89mL,n1=1

Conc. of NH3, M2=?, V2=64.7mL,n2=2

M2=(M1V1n2/n1V2) = 1.50*32.89*2/1*64.7 = 1.525M

The concentration of unknown NH3 solution = 1.525M

Ag+ (aq) + Cl- (aq) --> AgCl (s)
1mole AgCl = 1mole Ag+

i.e., 143.32g of AgCl contain 107.86g of Ag+

then 45.4mg=0.0454g of AgCl contain 107.86g/mol/143.32g/mol*0.0454g =0.0341g = 34.16mg of Ag+

Mass of silver ion in original 500mL of sample = 34.16mg

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