Question

4. To 43.4 mL of 0.221 M K₂CrO₄ solution are added 71.8 mL of 0.527 M ZnCrO₄. Calculate the molar concentrations of each ion present in the combined solutions.

7. A 30.0 mL sample containing citric acid (H₃C₆H₅O₇), a triprotic acid, is titrated (neutralized quantitatively) with a solution of 0.106 M KOH. The titration requires 26.5 mL of the KOH solution. Calculate the molar concentration of the citric acid solution. Also, identify the salt formed in the reaction and calculate its molar concentration. Assume solution volumes are additive.

Please help and explain the process to solving. I'm so confused, thanks in advance! :)

Answer 1

4 . K2CrO4(aq) → 2K+ (aq) + CrOÇ (aq) If 43.4mL 0.221MK,CrO4 and 71.8mL 0.527 M ZnCrO4 mixed then concentrations of all the ions [CrơJ-434mLx0.22mL + 71.8mL×0.527A [T]= [Zn2+]= 43.4mL+0.52mL CrO, 43.4mI+71.8mL 10, 41 2M Cro - +2x43.4mLx0.221M K* 43.4mL+71.8mL 二10.329M Zn2+