Calculate the ka for the acid

Reference no: EM13176299

The neutralization of an acid with a base yields a salt (and usually water) in aqueous solution. A)Calculate the pH when 35.0 mL of 0.471 M perchloric acid is mixed with 35.0 mL of 0.471 M sodium hydroxide solution at 25 °C. pH=? B)Calculate the pH when 35.0 mL of 0.471 M of a certain monoprotic weak acid, HA, is mixed with 35.0 mL of 0.471 M sodium hydroxide solution at 25 °C. For HA, the Ka is 6.5× 10-5. pH=? Calculate the concentrations of all species in a 0.970 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10-2 and Ka2 = 6.3× 10-8. [Na^+]=? [SO3 ^2-]=? [HSO3^-]=? [H2SO3]=? [OH^-]=? [H^+]=? NH3 is a weak base (Kb = 1.8 × 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.054 M in NH4Cl? pH=? Given that Ka for HBrO is 2.8 × 10-9 at 25 °C, what is the value of Kb for BrO- at 25 °C? Kb=? Given that Kb for C6H5NH2 is 1.7 × 10-9 at 25 °C, what is the value of Ka for C6H5NH3 at 25 °C? Ka=? For the diprotic weak acid H2A, Ka1 = 4.0 × 10-5 and Ka2 = 5.1 × 10-7. What is the pH of a 0.0550 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution? pH=? [H2A]=?M [A^2-]=?M Enough of a monoprotic acid is dissolved in water to produce a 1.59 M solution. The pH of the resulting solution is 2.88. Calculate the Ka for the acid. Ka=?

Reference no: EM13176299

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