Given one of the following solution: 50.00mL of 0.10M of K2CrO4 answer the following.
1. How do you prepare the solution?
2. What volume (mL) of your solution contains 5.00X10(-4) moles of the solute?
3. What volume of your solution contains 1.00g of the solute?
4. What is the new molarity of a solution made by pipeting 5.00mL of your solution and diluting 95.00mL of deionized water?
5. What of your solution is required to react with 10.00mL of 0.10M Pb(NO3)2?
*Can anyone help me out. I have another 5 problems to do on my own. I need some help with how to go about doing these problems. First one posted here.
To answer the given questions, let's break down each one and explain how to solve them step by step:
1. How do you prepare the solution?
To prepare a solution, you need to use the given information: 50.00 mL of 0.10 M K2CrO4. Here's how to prepare the solution:
a. Measure 50.00 mL of deionized water using a graduated cylinder.
b. Weigh out the appropriate amount of K2CrO4 to make a 0.10 M solution. To calculate this, you need to know the molar mass of K2CrO4, which is 194.2 g/mol. Multiply 0.10 M by 50.00 mL to get the required number of moles. Then multiply the moles by the molar mass to find the grams required.
c. Dissolve the measured amount of K2CrO4 in the measured volume of deionized water.
d. Mix the solution thoroughly to ensure proper dissolution.
2. What volume (mL) of your solution contains 5.00 × 10^(-4) moles of the solute?
To answer this question:
a. Calculate the molarity of the solution. Molarity (M) is defined as moles of solute per liter of solution. Since we know the moles and the volume in liters, we can directly use the formula M = moles/volume (in L).
b. Rearrange the formula to solve for the volume (in mL) using the given moles and molarity.
3. What volume of your solution contains 1.00 g of the solute?
To solve this question:
a. Convert the mass of the solute (K2CrO4) to moles by dividing it by the molar mass of K2CrO4.
b. Use the molarity formula (M = moles/volume) to convert moles of solute to volume (in L).
c. Convert the volume to mL.
4. What is the new molarity of a solution made by pipetting 5.00 mL of your solution and diluting it with 95.00 mL of deionized water?
For this question,
a. Calculate the moles present in the initial 5.00 mL of the solution using the molarity formula (moles = Molarity × Volume).
b. Calculate the final volume of the diluted solution (5.00 mL + 95.00 mL = total volume).
c. Use the molarity formula (M = moles/volume) to calculate the new molarity of the diluted solution.
5. What volume of your solution is required to react with 10.00 mL of 0.10 M Pb(NO3)2?
To answer this question:
a. Write the balanced chemical equation for the reaction between K2CrO4 and Pb(NO3)2.
b. Use the stoichiometry of the balanced equation to determine the molar ratio between K2CrO4 and Pb(NO3)2.
c. Calculate the number of moles of Pb(NO3)2 using the molarity formula (moles = Molarity × Volume).
d. Use the molar ratio from step b to determine the moles of K2CrO4 required.
e. Use the molarity formula (M = moles/volume) to calculate the required volume of K2CrO4 solution.
Remember, it's essential to show all the steps and unit conversions in your calculations to ensure accuracy. Let me know if you need further assistance with additional problems.
1. To prepare the solution, you would follow these steps:
a. Measure 50.00 mL of deionized water using a graduated cylinder or volumetric flask.
b. Weigh out the required amount of K2CrO4, which would be calculated based on the desired concentration and volume.
c. Add the weighed K2CrO4 to the measured deionized water.
d. Stir or shake the container to ensure proper mixing and dissolution of the solute.
e. Finalize the solution by adding more deionized water if necessary, to reach the desired final volume of 50.00 mL. Ensure that thorough mixing occurs.
2. To find the volume (mL) of the solution that contains 5.00 × 10^(-4) moles of the solute:
a. Use the formula: Moles = Concentration × Volume
b. Rearrange the formula to solve for Volume: Volume = Moles / Concentration
c. Plug in the given values: Moles = 5.00 × 10^(-4) mol and Concentration = 0.10 M
d. Calculate the volume of the solution using the formula: Volume = (5.00 × 10^(-4) mol) / (0.10 mol/L)
3. To find the volume of the solution that contains 1.00g of the solute:
a. Convert the mass of the solute to moles using its molar mass.
b. Use the formula: Moles = Mass / Molar Mass
c. Plug in the given values: Mass = 1.00 g and Molar Mass (K2CrO4) = 194.19 g/mol
d. Calculate the moles of the solute.
e. Use the mole-to-volume relationship from part 2 to calculate the volume of the solution.
4. To find the new molarity of the solution made through pipetting and dilution:
a. Calculate the moles of K2CrO4 in the original solution by using the formula from part 2.
b. Use the formula: Molarity = Moles / Volume
c. Plug in the given values: Moles from step a and Volume = 5.00 mL
d. Calculate the molarity of the original solution.
e. Use the dilution formula: M1V1 = M2V2
f. Plug in the given values: M1 (initial molarity) = calculated molarity, V1 (initial volume) = 5.00 mL, V2 (final volume) = 100.00 mL (5.00 mL + 95.00 mL)
g. Solve for M2 (final molarity) using the formula from step e.
5. To determine the amount of the given solution required to react with 10.00 mL of 0.10M Pb(NO3)2:
a. Write the balanced chemical equation for the reaction between K2CrO4 and Pb(NO3)2.
b. Use the stoichiometric ratios from the balanced equation to determine the ratio of moles between K2CrO4 and Pb(NO3)2.
c. Use the formula: Moles = Concentration × Volume
d. Plug in the given values: Concentration = 0.10 M and Volume = 10.00 mL
e. Calculate the moles of Pb(NO3)2 reacting.
f. Use the stoichiometric ratio from step b to calculate the moles of K2CrO4 required.
g. Use the formula from step 2 to find the volume of the given solution required.