Calculate the ${H^ + }$ ion concentration in a $1.00\,(M)$ $\,HCN\,$ litre solution $({K_a} = 4 \times {10^{ - 10}})$
Calculate the ${H^ + }$ ion concentration in a $1.00\,(M)$ $\,HCN\,$ litre solution $({K_a} = 4 \times {10^{ - 10}})$
- A
$4 \times {10^{ - 14}}\,mole/litre$
- B
$2 \times {10^{ - 5}}\,mole/litre$
- C
$2.5 \times {10^{ - 5}}\,mole/litre$
- D
None of these
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The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$
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- [AIPMT 1999]
Which of the following base is weakest
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- [IIT 2015]
The $pH$ of $0.1$ $M$ solution of cyanic acid $(HCNO)$ is $2.34$. Calculate the ionization constant of the acid and its degree of ionization in the solution.
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