50.00 mL of a solution containing 0.080 M H2SO4, and 0.20 M KIO3  Calculate the mass of potassium iodate required.

#9. In a titration experiment, 15.00 mL of 0.05000 M NaOH solution neutralizes 20.00 mL of H2SO4 solution. (a) Show and balance the reaction between NaOH and H2SO4. (b) What is the molarity of the H2SO4 solution?

Solid potassium hydroxide is slowly added to 75.0 mL of a 0.117 M lead(II) cyanide solution until the concentration of hydroxide ion is 0.0412 M. The percent of lead ion remaining in solution is %.

Solid potassium chromate is slowly added to 125 mL of a 0.440 M barium nitrite solution until the concentration of chromate ion is 0.0127 M. The percent of barium ion remaining in solution is   %?

4) A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055 M NaOH solution using phenolphthalein as theindicator. (a) If 19.60 mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)