Question

According to the following reaction: KHP + NaOH a NaKP + H_2O What is the concentration of the NaOH if it look 42.52 mL to titrate 0.835 g of KHP? (MM KHP = 204.2 g/mol) According to the following equation, how many ml of 0.15 M NaOH would be needed to titrate 10.00 ml of 0.500 M HCl? HCl + NaOH a NaCI + H_2O What is the pH of a 0.33 M solution of HCl? What is the [H+] of a solution with a pH of 2.1? Which of the following would be appropriate conjugate acid/base systems for a butler? NH/NH_4^+ HC_ H_3O_/NaC_ H_ O_ HCl/naOH What is chemical equilibrium? What are chemical kinetics? What does a change in temperature do to the kinetics of a reaction? What does a change in concentration do to the kinetics of a reaction? What is a catalyst and how does it work? Understand activation energy. According to the following equation, what would happen to the concentration of each of the species if the concentration of N_2O_5 were increased? If the concentration of NO_2 were decreased? If the pressure were increased? 2 N_2O_3 (g) beta a 4 NO_2(g) + O_2 (g) According to the equation above, what would be the equilibrium expression? What would be the equilibrium constant if [N_2 O_] = 0.50 M, [NO_] = 0.100 M, and [O_] = 0.025 M? Write the equilibrium expression for the following chemical reaction: CaCO_3 (s) beta a CaO (s) + CO_2 (g)

Answer 1

M_1 V_1 = M_2 V_2 M_2 = wt/MM times 1000/V (here V is V_2) rightarrow M_2 = wt/mm times 1000/V_2 rightarrow M_2 V_2 = wt/mm times 1000 rightarrow M_1 V_1 = M_2 V_2 = 0.835/204.2 times 1000 M_1 V_1 = 4.089 rightarrow M_1 = 4.089/V_1 = 4.089/42.52 rightarrow M_NaoH = 0.096 M Morality of Hcl given = 0.33 M rightarrow [H^+] = 0.33 = 3.3 times 10^-1 therefore p^H = -log [H^+] = -log [3.3 times 10^-1] = 0.48 p^H = 0.48 p^H = -log [H^+] = 2.1 rightarrow [H^+] = 10^-2.1 therefore [H^+] = 0.008 M