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)

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 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)

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]

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 ?

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) .

When 0.01 M HCl solution is added to 0.01 M Pb(NO_3)_2 solution, will a precipitate of PbCl_2 be formed or not? K_(sp)=1.6xx10^(-5) .

How many moles of NH_(3) must be added to 1 litre of 0.1 M AgNO_(3) solution to reduce Ag^(+) concentration to 2xx10^(-7) " M "K_(d) [Ag (NH_(3))_(2)^(+)] = 6.8 xx10^(-8) .

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 ?

1 mole of AgNO_(3) is added to 10 litre of 1 M NH_(3) . What is the concentration of Ag(NH_(3))^(+) in solution? [Given : For Ag(NH_(3))_(2)^(+),K_(f_(1))=2.0xx10^(3),K_(f_(2))=10^(3) ]