In each of these strong-acid - strong-base titrations, determinethe volume of ti

Question

In each of these strong-acid - strong-base titrations, determinethe volume of titrant that would effect a neutralization. (a) 0.016 L of0.72 M HCl titrated with0.48 M NaOH
_________________ L

(b) 49.3 mL of 0.75 M NaOH titrated with 0.68 M HCl
2 mL

(c) 21.3 mL of 0.97 M H2SO4 titratedwith 0.68 M KOH
3 mL

(d) 0.063 L of 0.27 M NaOH titrated with 0.22 M H2SO4
4 L (a) 0.016 L of0.72 M HCl titrated with0.48 M NaOH
_________________ L

(b) 49.3 mL of 0.75 M NaOH titrated with 0.68 M HCl
2 mL

(c) 21.3 mL of 0.97 M H2SO4 titratedwith 0.68 M KOH
3 mL

(d) 0.063 L of 0.27 M NaOH titrated with 0.22 M H2SO4
4 L

Explanation / Answer

(a)   Molarity, M1 = 0.72 M    Volume, V1 = 0.016 L Molarity, M2 = 0.48 M Volume of NaOH required , V2 = M1 V1 /  M2                                                  = 0.72 M * 0.016 L / 0.48 M                                                   =0.024 L (b) Similarly, Volume of HCl required, V2 = 49.3 mL * 0.75 M / 0.68 M (c) Volume of KOH required, V2 = 21.3 mL * 0.97 M / 0.68 M (d) Sulfuric acid is a diprotic acid. So two moles of NaOH arerequired to neutralize one mole of acid. Hence moles of NaOH, n1 = 2 moles of H2SO4, n2 = 1 M1 V1   /   n1   =   M2 V2 / n2 Volume of H2SO4, V2 = M1 V1 n2 / (n1M2)                                     =0.27 M * 0.063 L * 1 / ( 2 * 0.22 M)                                     =0.0386 L

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