Additional Practice Titrations 1) Calculate how much 0.100M HCl is needed to com

Question

Additional Practice Titrations 1) Calculate how much 0.100M HCl is needed to completely neutralize 10.0 mL of 0.150M KOH. (15.0mL) 2) Sketch the curve for the titration of 100 mL of a 0.10M weak acid (K.-1.0x 101) with 0.20M strong base. On the same axis, sketch the titration curve for the same volume and concentration of HCl. (Be sure to include pH of the equivalence point for each acid, the volume of strong base at the equivalence point, the volume of base and pH at the mid point, the initial pH of the solution, the pH of the system after a large excess of base has been added.) 3) Calculate the pH of each of the following solutions 1.00 mL of 0.150M formic acid plus 2.00mL of 0.100M NaOH. (use you book to determine the Ka for formic acid) (12.22) a.

Explanation / Answer

1)

Reaction is

KOH + HCl..............> KCl + H2O

one mole KOH react with one mole HCl to form one mole KCl and one mole H2O.

At neutralization point,

Va * Sa = Vb * Sb

Va * 0.100 M = 10.0 ml * 0.150 M

Va = 15.0 ml

so volume of HCl needed = 15.0 ml.

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