Among the solubility rules is the statement that carbonates, phosphates, borates, arsenates, and arsenites, except those of the ammonium ion and the alkali metals are insoluble.

K = [C a^{2 +}] [C O_{3}^{2 -}], K > 1

,
2.

K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K > 1

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K = [C a^{2 +}] [C O_{3}^{2 -}], K = 1

,
2.

K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K < 1

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K = [C a^{2 +}] [C O_{3}^{2 -}], K > 1

,
2.

K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K = 1

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K = [C a^{2 +}] [C O_{3}^{2 -}], K < 1

,
2.

K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K > 1

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Solution

The correct option is D 1. $K = [C a^{2 +}] [C O_{3}^{2 -}], K < 1$ ,
2. $K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K > 1$
$C a C O_{3} (s) ⇌ C a^{2 +} (a q) + C O_{3}^{2 -} (a q)$
$K = [C a^{2 +}] [C O_{3}^{2 -}], K < 1$
$3 B a^{2 +} (a q) + 2 P O_{4}^{3 -} (a q) ⇌ B a_{3} (P O_{4})_{2} (s)$
$K = \frac{1}{[B a^{2 +}]^{3} [P O_{4}^{3 -}]^{2}}, K > 1$

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Similar questions

For $C u^{2 +}$ ion in $[C u (H_{2} O)_{4} (e n)]^{2 +}, [C u (H_{2} O)_{2} (e n)_{2}]^{2 +}$ and $[C u (e n)_{3}]^{2 +}$ with the stability constant $k_{1}, k_{2}$ and $k_{3}$ respectively, which of the following holds true?

Q. For the hypothetical reaction, the equilibrium constant (k) values are given

A \to B (k = k_{1}) B \to C (k = k_{2}) C \to D (k = k_{3})

What is the value of equilibrium constant for

A \to D

Q. The equilibrium constants for the following are:

N_{2} + 3 H_{2} ⇌ 2 N H_{3} K_{1}

N_{2} + O_{2} ⇌ 2 N O K_{2}

H_{2} + \frac{1}{2} O_{2} \to H_{2} O K_{3}

The equilibrium constant (K) of the reaction:

2 N H_{3} + \frac{5}{2} O_{2} K ⇌ 2 N O + 3 H_{2} O,

will be

The equilibrium constants for the reactions are:

$H_{3} P O_{4}_{1} H^{+} + H_{2} P O_{4}^{-}; K_{1} H_{2} P O_{4}^{-}_{2} H^{+} + H P O_{4}^{2 -}; K_{2} H P O_{4}^{2 -}_{3} H^{+} + P O_{4}^{3 -}; K_{3}$

The equilibrium constant for, $H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{3 -}$ will be:

The following equilibrium constants are given

$N_{2} + 3 H_{2} ⇌ 2 N H_{3}; K_{1}$

$N_{2} + O_{2} ⇌ 2 N O; K_{2}$

$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O; K_{3}$

The equilibrium constant for the oxidation of $N H_{3}$ by oxygen to give $N O$ is:

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Among the solubility rules is the statement that carbonates, phosphates, borates, arsenates, and arsenites, except those of the ammonium ion and the alkali metals are insoluble.

The correct option is D 1. K=[Ca2+][CO2−3],K<1,2. K=1[Ba2+]3[PO3−4]2,K>1CaCO3(s)⇌Ca2+(aq)+CO2−3(aq)K=[Ca2+][CO2−3],K<13Ba2+(aq)+2PO3−4(aq)⇌Ba3(PO4)2(s)K=1[Ba2+]3[PO3−4]2,K>1