A weak base, `B`, has basicity constant `K_(b)=2xx10^(-5)`. The `pH` of any solution in which `[B]=[BH^(+)]` isA. `4.7`B. `7.0`C. `9.3`D. `9.7`

A weak base, `B`, has basicity constant `K_(b)=2xx10^(-5)`. The `pH` o

1.	A weak base, `B`, has basicity constant `K_(b)=2xx10^(-5)`. The `pH` of any solution in which `[B]=[BH^(+)]` isA. `4.7`B. `7.0`C. `9.3`D. `9.7`
Answer» Correct Answer - C `B+H_(2)OhArrBH^(+)+OH^(-)` `K_(b)=([BH^(+)][OH^(-)])/([B])` or `K_(b)=[OH^(-)]` `POH=5-log2` `:. pH=14-pOH=9+log2=9.3`

Discussion

No Comment Found

Related InterviewSolutions

Which of the following salts will give highest `pH` in water?A. `KCl`B. `Nacl`C. `Na_(2)CO_(3)`D. `CuSO_(4)`
The `pH` of `0.1 M` solution of the following salts increases in the orderA. `NaClltNH_(4)ClltNaCNltHCl`B. `HClltNH_(4)ClltNaClltNaCN`C. `NaCNltNH_(4)ClltNaClltHCl`D. `HClltNaClltNaCNltNH_(4)Cl`
Lemon juice normally has a `pH` of `2`. If all the acid the lemon juice is citric acid and there are no citrate salts present, then what will be the citric acid concentration `[Hcit]` in the lemon juice? (Assume that only the first hydrogen of citric acid is important) `HCithArrH^(+)+Cit^(-)`, `K_(a)=8.4xx10^(-4) mol L^(-1)`A. `8.4xx10^(-4) M`B. `4.2xx10^(-4) M`C. `16.8xx10^(-4) M`D. `11.9xx10^(-2) M`
If an aqueous solution at `25^(@)C` has twice as many `OH^(-)` as pure water its `pOH` will beA. `6.699`B. `7.307`C. `7`D. `6.98`
`pOH` of `H_(2)O` is `7.0` at `298K`. If water is heated at `350 K`, which of the following statement should be true?A. `pOH` will decrease.B. `pOH` will increase.C. `pOH` will remain `7.0`.D. concentration of `H^(+)` ions will increase but that of `OH^(-)` will decrease.
`10 mL` of `10^(-6) M HCl` solution is mixed with `90mL H_(2)O`. `pH` will change approximately:A. By one unitB. By `0.3` unitC. By `0.7` unitD. By `0.1` unit
`10ml` of `1 M H_(2)SO_(4)` will completely neutraliseA. `10 ml` of `1M NaOH` solutionB. `10 ml` of `2 M NaOH` solutionC. `5 ml` of `2 M KOH` solutionD. `5 ml` of `1 M Na_(2)CO_(3)` solution
The `pH` of an aqueous solution of `0.1 M` solution of a weak monoprotic acid which is `1%` ionised isA. `1`B. `2`C. `3`D. `11`
Three reactions involving `H_(2)PO_(4)^(-)` are given below `I. H_(3)PO_(4)+H_(2)OrarrH_(3)O^(+)+H_(2)PO_(4)^(-)` `II. H_(2)PO_(4)^(-)+H_(2)OrarrHPO_(4)^(2-)+H_(3)O^(+)` `III. H_(2)PO_(4)^(-)+OH^(-)rarrH_(3)PO_(4)+O^(2+)` In which of the above does `H_(2)PO_(4)^(-)` act as an acid?A. `II` onlyB. `I` and `II`C. `III` onlyD. `I` only
The conjugate base of `H_(2)PO_(4)^(-)` is :A. `HPO_(4)^(2-)`B. `P_(2)O_(5)`C. `H_(3)PO_(4)`D. `PO_(4)^(3-)`

A weak base, `B`, has basicity constant `K_(b)=2xx10^(-5)`. The `pH` of any solution in which `[B]=[BH^(+)]` isA. `4.7`B. `7.0`C. `9.3`D. `9.7`

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment