Ionic Product of Water

The conjugate base of water is 

The conjugate acid of water is 

The ionic product of water _____ if a few drops of acid or base are added to it.

Calculate the ${\mathrm{K}}_{\mathrm{w}}$ of water at $90°\mathrm{C}$, if pure water has $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]={10}^{-6 }\mathrm{M}$  at the given temperature.

Which of these statements is correct about pure water?

The pH of pure water at $25°\mathrm{C}$ and $35°\mathrm{C}$are $7$ and $6$ respectively. What is the heat of formation of water from ${\mathrm{H}}^{+}$ and ${\mathrm{OH}}^{-}$? 

${\mathrm{K}}_{\mathrm{b}}$ for weak base $\mathrm{B}$ is $1.0\times {10}^{-6}$ then hydrolysis constant for the reaction
${\mathrm{B}}^{+}+{\mathrm{H}}_2\mathrm{O}\stackrel{\mathrm{}}{\rightleftharpoons }\mathrm{}\mathrm{B}\mathrm{O}\mathrm{H}+{\mathrm{H}}^{+}$ is

The sodium salt of a weak acid is hydrolysed to the extent of 3% in 0.1 M solution in water at $25°\mathrm{C}$ . If ${\mathrm{K}}_{\mathrm{a}}$ for weak acid is $1.3\times 10^{-10}$ . The ionic product of water is

Hydrolysis constants of two salts ${\text{K}}_{\text{hA}}$ and ${\text{K}}_{\text{hB}}$ of weak acids HA and HB are $10^{-8}$ and $10^{-6}$ . If the dissociation constant of third acid HC is $10^{-2}$ . The order of acidic strength of three acids will be

At $90°\mathrm{C}$ , pure water has $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=10^{-6}$ mol $\mathrm{l}\mathrm{i}\mathrm{t}\mathrm{r}{\mathrm{e}}^{-1}$ . What is the value of ${\mathrm{K}}_{\mathrm{w}}$ at $90°$ C?

Which of the following constitutes a set amphoteric species –

If ${\mathrm{K}}_{\mathrm{a}}={10}^{–5}$ for a weak acid, then ${\mathrm{p}\mathrm{K}}_{\mathrm{b}}$ for its conjugate base would be -

Equal volumes of three strong acid solutions of $\mathrm{p}\mathrm{H}\mathrm{ }3,\mathrm{ }4$ and $5$ are mixed in a vessel. What will be the ${\mathrm{H}}^{+}$ ion concentration in the mixture?

At a certain temperature, the value of$\mathrm{ }{\mathrm{p}\mathrm{K}}_{\mathrm{w}}$ is $13.4$ and the measured $\mathrm{p}\mathrm{H}$ of a solution is $7$. The solution is:

At a certain temperature, pure water has hydronium ion concentration equal to ${10}^{–6.5\mathrm{ }}\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{e}$ ${\mathrm{L}}^{–1}$. The value of ${\mathrm{K}}_{\mathrm{w}}$ at this temperature will be -

At $90°\mathrm{ }\mathrm{C}$, pure water has $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]={10}^{–6}\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }{\mathrm{L}}^{–1}$. What is the value of ${\mathrm{K}}_{\mathrm{w}}$ at $90°\mathrm{ }\mathrm{C}$ -

Which of the following is incorrect for pure water at the given temperature?

(At the given temperature ${\mathrm{K}}_{\mathrm{w}}$ for water is  $4\mathrm{ }\times \mathrm{ }{10}^{–14}$)
 

At what molar concentration of HCl will its aqueous solution have an [H⁺] to which equal contribution come from HCl and H₂O at 90^oC.

[K_w of H₂O = 10^-12 M² at 90^oC]

Which one of the following statements does not define the characteristic property of water- "Water is a universal solvent" ?

An aqueous solution in which the ${\mathrm{H}}^{+}$ ion concentration is greater than ${10}^{-7}$ M is said to be