# Chemistry

posted by .

A 35ml 0.1M AgCl solution is mixed with 15ml 0.25M MgCl2 solution. Calculate the moles and molarities of the Ag+, NO3-,Mg2+, and Cl- ions in the solution mixture.

• Chemistry -

I think it was 35 mL of 0.1M AgNO3, not AgCl. When the two solutions are mixed the reaction is:
2AgNO3(aq) + MgCl2(aq) ---> AgCl(s) + Mg(NO3)2(aq)
Moles of AgNO3 = (0.035L)(0.1mol/L) = 0.0035 moles of AgNO3. Moles of Ag+ ion = 0.0035 also.
Likewise, moles of MgCl2 = (0.015 L)(0.25 mol/L) = 0.00375 mol MgCl2. Moles of Cl- ion = (2)(0.00375) = 0.0075
The mole ratio of AgNO3 to MgCl2 is 2/1. However, the ratio used is 0.0035/0.00375 which is much smaller. That means AgNO3 is the limiting reagent (gets used up) in forming the precipitate AgCl. Some of the chloride ion is also used:
0.0075 - 0.0035 = 0.0040 moles of Cl- left in slution.
Total volume of solution = 15 + 35 = 50 mls = 0.050 L
From what I have shown you so far,
Final concentration of Ag+ = 0
Final concentration of Cl- = 0.0040 mol/0.050 L, or [Cl-] = 0.080 mol/L
Final concentration of NO3- = 0.0035 mol/0.050L = 0.070 mol/L
The final concentration of Mg+2, I leave to you.

## Similar Questions

1. ### Chemistry

A solution was prepared by adding 15mL of 0.129 M KI, 5mL of 0.1 M Na2S2O3, 1mL of starch solution, and 15mL of 0.125 M (NH4)2S2O8. Calculate the concentration of (M) of I in the final mixture before the chemical reaction.
2. ### Chemistry

Question: you have a clear, colorless aqueous sample in a beaker that contains either CO2^-2(aq) or C^-1(aq) or a mixture of both ions. the following aqueous reagents are available: NaCl, HNO3, and AgNO3. describe a procedure that …
3. ### Chemistry

A solution is prepared by mixing 0.12 L of 0.12 M sodium chloride with 0.22L of a 0.19M MgCl2 solution.What volume of a 0.22 M silver nitrate solution is required to precipitate all the Cl- ion in the solution as AgCl ?
4. ### AP Chem

A sample of solid KCl (potassium chloride) weighing 0.500 g is mixed with an unweighed sample of solid MgCl2 (magnesium chloride) and the mixture is then completely dissolved in water to form a clear solution. An aqueous solution of …
5. ### chemistry

A sample of solid KCl (potassium chloride) weighing 0.500 g is mixed with an unweighed sample of solid MgCl2 (magnesium chloride) and the mixture is then completely dissolved in water to form a clear solution. An aqueous solution of …
6. ### chemistry

15ml of 0.325M NaOH is delivered into 35ml HOBr solution of unknown concentration.The pH of the final solution is 7.48. Ka for HOBr is 2.0 x 10-9at 25C. Find the number of moles of OBr- and HOBr in the final solution.
7. ### Chemistry

Pb(NO3)2(aq) 2 x 10-3 M and Na2SO4(aq) 2 x 10-3 M Identify the ions that are present in each solution, and calculate their concentrations. If 1 L of each solution are mixed, will a precipitate be formed?
8. ### chemistry

A beaker contain 300.ml of a 0,20 M Pb(NO3) solution. If 200 ml of 0,20M solution og MgCl2 is added to the beaker, What will be the concentration of Pb2+ ions in the resulting solution
9. ### chemistry

find the mass of silver chloride formed from 33.2ml of a 0.100M solution of silver nitrate and 200ml of 0.200M solution of calcium chloride solution Solution plan:use mass to mass calculations mass of AgNO3-moles of AgNO3-moles of …
10. ### chemistry

A) A solution was prepared by dissolving 1.113 g of MgCl2 into water and made up to 50.0 ml, calculate the molar concentration of the solution. B) A 250.0 ml of 0.50 M solution of Na3PO2 solution was prepared by diluting 2.5 M of stock …

More Similar Questions

Post a New Question