If 4.oo mL of 0.0250 M CuSO4 is diluted to 10.0 mL with pure water, what is the molar concentration of copper (II) sulfate in the dilute solution?
A 10.0-mL sample of 2.56 M HCL is diluted with water to 250. mL.
What is the concentration of HCl in the diluted solution?
Concentration of HCL______________________
What is the pH of the dilute solution?
ph of the dilute solution_______________________© BrainMass Inc. brainmass.com December 24, 2021, 4:55 pm ad1c9bdddf
SOLUTION This solution is FREE courtesy of BrainMass!
1. Dilution ==> V * M = V' * M'
where M = Molarity before dilution
V is volume of solution before dilution
Or, 4*0.025 = 10*M' which gives M' = 4*0.025/10 = 0.01M ---Answer
2. The most important thing to remember concerning dilution is that you are adding only solvent. You are not adding solute when you dilute. Therefore:
moles of solute before dilution = moles of solute after dilution
Molarity = moles of solute/volume of solution in liters
Moles of solute = Molarity*liters of solution = 2.56*10 = 25.6
New molarity = 25.6/250 = 0.1024 M ----Answer
3.pH is a measure of the hydrogen ion concentration, [H+]
pH is calculated using the following formula:
pH = -log_10 [H+]
Here we need to find the pH of a 0.1024M solution of HCl
0.1024 mol L of HCl produces 0.1024 mol L-1 H+ since HCl is a strong acid that fully dissociates.
thus, [H+] = 0.1024
pH = -log_10[0.1024] = 0.9897 ---Answer© BrainMass Inc. brainmass.com December 24, 2021, 4:55 pm ad1c9bdddf>