Ionic Product of Water

Calculate the percent error in the hydrogen-ion concentration made by neglecting the ionization of water in a $1\times {10}^{-6} \mathrm{M} \mathrm{NaOH}$ solution.

The conjugate base of water is 

The conjugate acid of water is 

How many litres of water must be added to $1$ litre of aqueous solution of $\mathrm{HCl}$ with a pH of $1$ to create an aqueous solution with pH of $2$?

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 ${\mathrm{OH}}^{-}$? 

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead precipitation of copper iodate? (For cupric iodate K_sp = 7.4 × 10^-8). If the value of Ionic product of CU(SO₃)₂ in the reaction mixture is Yx 10^-9. Find Y.

The ${\mathrm{K}}_{\text{sp}}$ of Mg $(\text{OH}{)}_2$ is $1\times 10^{-\text{12}}.$ A 0.01 M $\text{MgC}{\text{l}}_2$ solution will precipitate at what limiting pH value?

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 $90°\mathrm{ }\mathrm{C}$ -

What is the concentration of ${\mathrm{A}\mathrm{g}}^{+}$ ion in a $1\mathrm{L}$ solution containing $0.02\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}$ of ${\mathrm{A}\mathrm{g}\mathrm{N}\mathrm{O}}_3$ and $0.14\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}$ of ${\mathrm{N}\mathrm{H}}_3$. For $\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2^{+},\mathrm{K}={10}^8$

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

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

What will be the result if 100 ml of 0.06 M Mg(NO₃)₂ solution is added to 50 ml of 0.06 M Na₂C₂O₄ solution. The K_sp of MgC₂O₄ (s) is 8.6 × 10^-5 M²

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" ?