When `0.1 m "mole"` of solid `NaOH` is added in `1 L` of `0.1 M NH_(3) (aq)` then which statement is going to be wrong?
`(K_(b)=2xx10^(-5), log 2=0.3)`

When 0.1 mole solid NaOH is added to 1 L of 0.01 M NH_3(aq) , then which statement is wrong ? ( K_b=2xx10^(-5) , log 2 =0.3)

How many moles of NaOH can be added to 1.0L solution of 0.10MNH_(3) and 0.10MN_(4)CI without changing in volume. (K_(b)for NH_(3)=1.8xx10^(-5))

Calculate the number of moles of NH_(4)Cl that should be added to one litre of "1.0 M "NH_(4)OH to prepare buffer solution with pH=9[K_(b)=2xx10^(-5)," take log"2=0.3]

Calculate the number of moles of NH_(4)Cl that should be added to one litre of "1.0 M "NH_(4)OH to prepare buffer solution with pH=9[K_(b)=2xx10^(-5)," take log"2=0.3]

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. b. How much NaOH should be added to 1L of the solution to change pH by 0.6.K_(b) =2xx10^(-5) .

Which of the following solutions when added to 1L of a 0.1 M CH_3COOH will cause no change in the pH of the solution K_a=1.8xx10^(-5) for CH_3COOH ?

Which of the following solutions when added to 1L of a 0.1 M CH_3COOH or in the pH of the solution K_a=1.8xx10^(-5) for CH_3COOH ?