The pH of $0.1\mathrm{M}$ ammonia solution ($K_b=1.8\times 10^{-5}$ at 298 K; use $[\mathrm{OH}{}^{-}]=\sqrt{K_{b}c}$, $\log 1.34=0.127$) is

More questions on pH of strong and weak acids and bases, mixtures

• 50 mL of 0.2 M HCl is mixed with 50 mL of 0.1 M NaOH. The pH of the resulting solution is nearest to. Use log 2=0.301 and log 3=0.477 where ... JEE Main level
• 40 mL of 0.1 M NaOH is mixed with 10 mL of 0.2 M HCl. The pH of the resulting solution is nearest to. Use log 2=0.301 and log 3=0.477 where ... JEE Main level
• The pH of 0.01 M solution of a weak acid with K_a=4x10^-6 (neglect water ionisation and use [H+]=sqrtK_ac) is. Use log 2=0.301 and log 3=0.4... JEE Main level
• A 0.1 M solution of a weak acid has degree of ionisation 0.01. If it is diluted to 0.025 M (assume alphall1), the new degree of ionisation i... JEE Main level
• Equal volumes of 0.1 M HCl and 0.1 M acetic acid (K_a=1.8x10^-5) are mixed. The pH of the mixture is nearest to (use log5=0.699) JEE Main level
• A 0.05 M solution of a weak monobasic acid has pH 3.30. Neglecting alpha against 1, the K_a of the acid is nearest to (10^-3.30=5.01x10^-4) JEE Main level