The solubility product of Ag2CrO4 in water a 298 K is 3.2× 10-11 . What will be the concentration of CrO42- ions in the saturate solution of Ag2CrO4 ?

Question

The solubility product of Ag2CrO4 in water a 298 K is 3.2× 10-11 . What will be the concentration of CrO42- ions in the saturate solution of Ag2CrO4 ? (A)  2× 10-4M  (B)  5.7× 10-5M  (C)  5.7× 10-6M  (D)  3.2× 10-11

Tardigrade Admin · Accepted Answer

For saturated solution of Ag 2 CrO 4, if solubility is ' s' mol L -1. Then undersetsAg 2 Cr O 4 leftharpoons underset2s2 Ag +(a q)+ underset s Cr O 42-(a q) Ks p =(2 s)2(s)=4 s3 Ks p =3.2 × 10-11 (given) ∴ 3.2 × 10-11 =4 s3 s3 =(3.2 × 10-11/4)=8 × 10-12 ∴ s =√8 × 10-12=2 × 10-4 M

Q. The solubility product of $A g_{2} C r O_{4}$ in water a $298 K$ is $3.2 \times 10^{- 11}$ . What will be the concentration of $C r O_{4}^{2 -}$ ions in the saturate solution of $A g_{2} C r O_{4}$ ?

$2 \times 10^{- 4} M$

$5.7 \times 10^{- 5} M$

$5.7 \times 10^{- 6} M$

$3.2 \times 10^{- 11}$

Q. The solubility product of Ag2​CrO4​ in water a 298K is 3.2×10−11 . What will be the concentration of CrO42−​ ions in the saturate solution of Ag2​CrO4​ ?

2×10−4M

5.7×10−5M

5.7×10−6M

3.2×10−11

For saturated solution of Ag2​CrO4​, if solubility is ' s′molL−1. Then sAg2​CrO4​​⇌2s2Ag+​(aq)+sCr​O42−​(aq) Ksp​=(2s)2(s)=4s3 Ksp​=3.2×10−11 (given) ∴3.2×10−11=4s3 s3=43.2×10−11​=8×10−12 ∴s=8×10−12​=2×10−4M

Q. The solubility product of $A g_{2} C r O_{4}$ in water a $298 K$ is $3.2 \times 10^{- 11}$ . What will be the concentration of $C r O_{4}^{2 -}$ ions in the saturate solution of $A g_{2} C r O_{4}$ ?

$2 \times 10^{- 4} M$

$5.7 \times 10^{- 5} M$

$5.7 \times 10^{- 6} M$

$3.2 \times 10^{- 11}$