What is the aq. Ammonia concentration of a solution prepared by dissolving 0.15 mole of `NH_4^+CH_3COO^-` in 1 L `H_2O` ?
`[K_(a(CH_3COOH))=1.8xx10^(-5)=K_(b(NH_3))]`

What is the concentration of CH_(3)COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1 L H_(2)O ? [K_(a(CH_(3)COOH))=1.8xx10^(-5)),K_(b(NH_(4)OH)=1.8xx10^(-5))]

What is the concentration of CH_(3)COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1 L H_(2)O ? [K_(a(CH_(3)COOH))=1.8xx10^(-5)),K_(b(NH_(4)OH)=1.8xx10^(-5))]

What is the concentration of CH_(3)COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1 L H_(2)O ? [K_(a) (CH_(3)COOH))=1.8xx10^(-5)),K_(b) (NH_(4)OH)=1.8xx10^(-5))]

What is the concentration of CH_(3)COOH(aq) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1L H_(2)O ? Report your answer after multiplying by 9xx10^(5) .

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

The pH of a solution containing 0.1 M CH_3COONa and 0.1 M (C_2H_5COO)_2 Ba will be K_a(CH_3COOH)=2xx10^(-5). K_a(C_2H_5COOH)=1.5xx10^(-5) :

What is [H^(+)] in mol//L of a solution that is 0.20 M in CH_(3)COONa and 0.1 M in CH_(3)COOH ? K_(a) for CH_(3)COOH is 1.8xx10^(-5) ?