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Chemistry-

General

Easy

Question

The ionic product of water is 10^–14 The H⁺ ion concentration in 0.1M NaOH solution is

10^–11M
10^–13M
10^–1M
10^–4M

The correct answer is: 10^–13M

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At certain temperature, the H⁺ ion concentration of water is 4 × 10^–7M then the value of Kw at the same temperature is

At certain temperature, the H⁺ ion concentration of water is 4 × 10^–7M then the value of Kw at the same temperature is

chemistry-General

At 25 $degree$ C , the hydroxyl ion concentration of a basic solution is 6.75 × 10^–3M .Then the value of Kw is

At 25 $degree$ C , the hydroxyl ion concentration of a basic solution is 6.75 × 10^–3M .Then the value of Kw is

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The $open square brackets O H to the power of minus end exponent close square brackets$ of 0.005 M H₂SO₄ is

The $open square brackets O H to the power of minus end exponent close square brackets$ of 0.005 M H₂SO₄ is

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The H⁺ ion concentration of a solution is 4×10^–5 M. Then the OH^– ion concentration of the same solution is

The H⁺ ion concentration of a solution is 4×10^–5 M. Then the OH^– ion concentration of the same solution is

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The least soluble compound (salt) of the following is

The least soluble compound (salt) of the following is

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To Ag₂CrO₄ solution over its own precipitate, $C r O subscript 4 end subscript superscript 2 minus end superscript$ ions are added. This results in

To Ag₂CrO₄ solution over its own precipitate, $C r O subscript 4 end subscript superscript 2 minus end superscript$ ions are added. This results in

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When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because

When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because

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Let the solubility of an aqueous solution of Mg(OH)₂ be ‘X’ then its K_sp is

Let the solubility of an aqueous solution of Mg(OH)₂ be ‘X’ then its K_sp is

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The molar solubility in mol.lit^-1 of a sparingly soluble salt MX₄ is S. The corresponding solubility product K_sp is given by the relation.

The molar solubility in mol.lit^-1 of a sparingly soluble salt MX₄ is S. The corresponding solubility product K_sp is given by the relation.

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Among the following statements a) If two salts have equal solubility then their solubility products are equal. b) BaSO₄ in more soluble in water than in dil.H₂SO₄ . c) When KI is added to PbI₂ , then the $[{P b}^{2 +}]$ decreases d) In any solution containing AgCl , the value of $[{A g}^{+}] [{C l}^{-}]$ is constant at constant temperature.

Among the following statements a) If two salts have equal solubility then their solubility products are equal. b) BaSO₄ in more soluble in water than in dil.H₂SO₄ . c) When KI is added to PbI₂ , then the $[{P b}^{2 +}]$ decreases d) In any solution containing AgCl , the value of $[{A g}^{+}] [{C l}^{-}]$ is constant at constant temperature.

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In which of the following, the solubility of AgCl will be maximum ?

In which of the following, the solubility of AgCl will be maximum ?

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At 298 K , the K_sp value of Fe(OH)₃ in aqueous solution is $3.8 \times 10^{- 38}$ The solubility of Fe³⁺ ions will increase when

At 298 K , the K_sp value of Fe(OH)₃ in aqueous solution is $3.8 \times 10^{- 38}$ The solubility of Fe³⁺ ions will increase when

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In the following reaction , $A g C l + K I \to K C l + A g I$ . As KI is added , the equilibrium is shifted towards right giving more AgI precipitate , because

In the following reaction , $A g C l + K I \to K C l + A g I$ . As KI is added , the equilibrium is shifted towards right giving more AgI precipitate , because

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Which of the following is most soluble ?

Which of the following is most soluble ?

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Which of the following has the lowest value of K_sp at 25°C ?

Which of the following has the lowest value of K_sp at 25°C ?

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