A solution of hydrogen peroxide was titrated with a solution of potassium permanganate (see reaction).  5 H 2O 2(aq) + 2 KMnO 4(aq) + 3 H 2SO 4 -> 5 O 2(g) + 2 MnSO 4(aq) + K 2SO 4(aq) + 8 H 2O(l)It required 75.00 mL of 0.1626 M KMnO 4 to titrate 3.564 g of the solution containing hydrogen peroxide. What was the mass percentage of H 2O 2 in the solution?

The calcium in a 200 mL sample of water sample was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus Cao (56.077 g/mol) was 26.7134 g. Calculate the Molarity of Ca. a. 0.005 M O b. 0.040 M O c. 0.100 M O d. 0.080 M O e. 0.010 M

50 mL of a 1.067 M solution of HCI was diluted to 250 mL. The diluted HCI solution was then titrated with an unknown concentration of KOH. It is found that an average volume of 24.20 mL of KOH is required to reach an endpoint in a titration with 25.00 mL of the dilute acid solution. The equation for the reaction is; H(aq) + OH(aq) →→> H₂O (1) The concentration of KOH is 0.2205 M Calculate the concentration of the KOH in g/L (you will need to find the formula weight of KOH to do this) 15| ΑΣΦ ? g/L

The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 5.43 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCI(aq) and passed over a reducing agent so that all the antimony is in the form Sb³*(aq). The Sb³+(aq) is completely oxidized by 28.0 mL of a 0.110 M aqueous solution of KBrO, (aq). The unbalanced equation for the reaction is Bro, (aq) + Sb³+(aq) → Br (aq) + Sb3+ *(aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: percentage of antimony: %