When solutions of silver nitrate and calcium chloride are mixed, silver chloride

Question

When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNOx (aq) + CaC12 (aq)–2AgCl(s) + Ca(NOx)2(aq) Part A What mass of silver chloride can be produced from 1.69 L of a 0222 M solution of silver nitrate? Express your answer with the appropriate units. Hints OH WA a O 8 ? mas of AgC Value Units Submit my answers Give Up | = Part B The reaction described in Part A required 3.29 L of calcium chloride. What is the concentration of this calcium chloride solution? Express your answer with the appropriate units. Hints

Explanation / Answer

0.222= no of molesof silver nitrate/1.69

no of moles of silver nitrate=0.222 x 1.69

=0.3751

no of moles=wieght/MW

0.3751=weight/169.87

weight=63.72g of Silver nitrate

you can see in the raection that AgNO3 and AgCl are in 1:1 ratio

hence 169.87g of AgNO3 will produce 143.32g AgCl(MW of AgCl)

hence 63.72g will produce xg

Xg=143.32x63.72/168.87=53.76g of AgCl

B) again looking at the ratio ,for every 2 moles of AgNO3, one mole of CaCl2 was used

hence for 169.87g of AgNO3 143.32/2g CaCl2 will be used

hence for 63.72g xg will be used

x=26.88g

Molarity=26.88/143.32x3.29

=0.057M

please do rate

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