Question

How many gram Agcl will be obtain when a solution containing 3.4gram AgNO3 react with 400ml 0.5 MHCL​

Answer 1

Explanation:

double replacement reactions involve the reaction between ionic compounds in solution and, in the course of the reaction, the ions in the two reacting compounds are “switched” (they replace each other). As an example, silver nitrate and sodium chloride react to form sodium nitrate and the insoluble compound, silver chloride.

AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq)(7.5.1)(7.5.1)AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq)

Because these reactions occur in aqueous solution, we can use the concept of molarity to directly calculate the number of moles of products that will be formed, and hence the mass of precipitates. In the reaction shown above, if we mixed 123 mL of a 1.00 M solution of NaCl with 72.5 mL of a 2.71 M solution of AgNO3, we could calculate the moles (and hence, the mass) of AgCl that will be formed as follows:

First, we must examine the reaction stoichiometry. In this reaction, one mole of AgNO3 reacts with one mole of NaCl to give one mole of AgCl. Because our ratios are one, we don’t need to include them in the equation. Next, we need to calculate the number of moles of each reactant:

0.123L×(1.00mole1.00L)=0.123molesNaCl(7.5.2)(7.5.2)0.123L×(1.00mole1.00L)=0.123molesNaCl

0.0725L×(2.71mole1.00L)=0.196molesAgNO3(7.5.3)