Consider the reaction: K2S(aq)+Co(NO3)2(aq)=2KNO3(aq)+CoS(s) what volume of 0.255 M K2S solution is required to completely react with 160 mL of 0.130 M

Co(NO3)2?

To determine the volume of the K2S solution required for the reaction, we can use the stoichiometry of the balanced equation to calculate the amount in moles.

First, let's write down the balanced equation:

K2S(aq) + Co(NO3)2(aq) -> 2KNO3(aq) + CoS(s)

From the balanced equation, we can see that the mole ratio between K2S and Co(NO3)2 is 1:1. This means that for every 1 mole of Co(NO3)2, we need 1 mole of K2S to react.

Now, let's calculate the amount of Co(NO3)2 used in moles:

moles of Co(NO3)2 = concentration x volume
= 0.130 M x 0.160 L
= 0.0208 moles

Since the mole ratio between Co(NO3)2 and K2S is 1:1, we need the same amount of moles of K2S to react:

moles of K2S = 0.0208 moles

Finally, we can calculate the volume of the 0.255 M K2S solution needed to react with the given amount of Co(NO3)2:

volume of K2S = moles / concentration
= 0.0208 moles / 0.255 M
= 0.0816 L

To convert the volume to milliliters:

volume of K2S = 0.0816 L x 1000 mL/L
= 81.6 mL

Therefore, 81.6 mL of the 0.255 M K2S solution is required to completely react with 160 mL of 0.130 M Co(NO3)2.

To find the volume of the K2S solution required to completely react with the Co(NO3)2 solution, we need to use the concept of stoichiometry and the balanced chemical equation.

1. Start by writing the balanced chemical equation for the reaction:
K2S(aq) + Co(NO3)2(aq) → 2KNO3(aq) + CoS(s)

2. Determine the stoichiometric ratio between K2S and Co(NO3)2 by looking at their coefficients in the balanced equation:
K2S : Co(NO3)2 = 1 : 1

3. Calculate the number of moles of Co(NO3)2 present in the given 160 mL solution. We can use the formula: moles = concentration (M) × volume (L). Convert milliliters to liters by dividing by 1000:
Moles of Co(NO3)2 = 0.130 M × (160 mL / 1000 mL/L)

4. Now, to react completely with Co(NO3)2, we need an equal number of moles of K2S. Use the stoichiometric ratio from step 2 to calculate the moles of K2S required:
Moles of K2S = Moles of Co(NO3)2

5. Finally, to find the volume of the 0.255 M K2S solution required, divide the moles of K2S by its concentration:
Volume of K2S solution = (Moles of K2S) / (0.255 M)

Performing the calculations:
Moles of Co(NO3)2 = 0.130 M × 0.160 L = 0.0208 moles
Moles of K2S required = 0.0208 moles
Volume of K2S solution = 0.0208 moles / 0.255 M

Therefore, the volume of the 0.255 M K2S solution required to completely react with 160 mL of 0.130 M Co(NO3)2 is approximately 0.082 L or 82 mL.

I have copied the equation without the phases to save space.

K2S + Co(NO3)2 = 2KNO3 + CoS
mols Co(NO3)2 = M x L = ?
Using the coefficients in the balanced equation, convert mols Col(NO3)2 to mols K2S. Since the coefficients are the same then mols Co(NO3)2 = mols K2S.
Then M K2S = mols K2S/L K2S. You know mols and M, solve for L and convert to mL if needed.