Consider the reaction: #K_2S_((aq))+Co(NO_3)_(2(aq)) -> 2KNO_(3(aq))+CoS_((s)) darr#. What volume of 0.220M #K_2S# solution is required to completely react with 160mL of 0.145M #Co(NO_3)_2#?

That much cobalt nitrate requires 105 mL of 0.220-M potassium sulfide solution to fully react.

For this double replacement reaction, start with the balanced chemical equation.

Calculate the moles of cobalt nitrate in the solution by utilizing its volume and molarity.

For the cobalt nitrate to react fully, 0.0232 moles of potassium sulfide must be present. Once more, use the molarity of the solution to calculate the volume you'd need.

The number of sig figs you provided for the volume of the cobalt nitrate solution, expressed in milliliters and rounded to two sig figs, will be the answer.

To solve this problem, you can use the stoichiometry of the reaction to determine the amount of K2S needed to react with the given amount of Co(NO3)2. First, calculate the moles of Co(NO3)2 using its molarity and volume. Then, use the mole ratio between Co(NO3)2 and K2S from the balanced equation to find the moles of K2S required. Finally, use the molarity and the moles of K2S to find the volume needed.

Moles of Co(NO3)2 = Molarity × Volume = 0.145 M × 0.160 L = 0.0232 moles

From the balanced equation, the mole ratio between Co(NO3)2 and K2S is 1:1. Therefore, moles of K2S required = 0.0232 moles.

Now, use the molarity of K2S to find the volume:

Volume = Moles / Molarity = 0.0232 moles / 0.220 M ≈ 0.1056 L

Convert the volume to milliliters:

Volume ≈ 0.1056 L × 1000 mL/L ≈ 105.6 mL

So, approximately 105.6 mL of 0.220 M K2S solution is required to completely react with 160 mL of 0.145 M Co(NO3)2.