When 35 {mL} of 0.15 {M} lead nitrate solution is mixed with 20 {mL} of 0.12 {M} chromic sulphate solution, ........ \times 10^{-5} moles of lead sulphate precipitate out. (Round off to the nearest integer). [16 Mar 2021 Shift 2]

JEE Main 16 March 2021 Shift 2 Solved Paper

Section: Chemistry

Question : 58 of 90

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When 35mL of 0.15M lead nitrate solution is mixed with 20mL of 0.12M chromic sulphate solution, ........ ×10−5 moles of lead sulphate precipitate out. (Round off to the nearest integer).

[16 Mar 2021 Shift 2]

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3Pb(NO3)2	+	Cr2(SO4)3	⟶	3PbSO4	+	2Cr(NO3)3
35‌mL	‌	20‌mL
0.15‌ML	‌	0.12‌ML
M×V	‌	20×0.12
35×0.15	‌	=2.4	‌	0	‌	0
=5.25

3Pb(NO3)2	+	Cr2(SO4)3	⟶	3PbSO4	+	2Cr(NO3)3
t=05.25m‌mol	‌	2.4	‌	0	‌	0
t=t‌5.25525	‌	2.4−1.7=0.7	‌	5.25
=0