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Determine the molar mass of the unknown acid

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Reference no: EM131445173

1. A 120.0 -mL sample of a solution that is 3.0×10-3M in AgNO3 is mixed with a 230.0 -mL sample of a solution that is 0.14 M in NaCN.

After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Express your answer using two significant figures.

B. A 0.5210 -g sample of an unknown monoprotic acid was titrated with 9.96×10-2 M NaOH. The equivalence point of the titration occurs at 23.88 mL .

Determine the molar mass of the unknown acid.

2. Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.

MX (Ksp = 1.30×10-38)

Reference no: EM131445173

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Determine the molar mass of the unknown acid : Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. MX (Ksp = 1.30×10-38)
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