Find the pH:
1) A 0.001M solution of HCl
2) A 7.98 x 10^-2 M solution of HNO3
3) 1098L of a solution containing 8.543moles of HBr
4) 120mL of a solution containing 0.005 grams of hydrochloric acid.
Please help me with these four. Out of 20 questions i only didn't understand these four is that good or bad:(? Please help step by step so i can understand:)
Thanks a bunch!!!!!!!!:D
1) HCl is a strong acid meaning that it is 100% ionized. Therefore,
pH = -log(HCl) = -lo(H^+) = ?
2) HNO3 is also a strong acid. This problem is worked the same way as number one.
3) Again, HBr is a strong acid. mols HBr = grams/molar mass. Then M = mols/L
4) Number four is worked the same as number three.
Sure! I'd be happy to help you step by step with each of these questions. Let's go through them one by one:
1) A 0.001M solution of HCl:
To find the pH of the solution, we need to use the equation for the dissociation of HCl in water: HCl → H+ + Cl-
Since the concentration of HCl is given as 0.001M, the concentration of H+ ions is also 0.001M.
To find the pH, we can use the equation pH = -log[H+]. Substituting the concentration of H+, we get: pH = -log(0.001) = 3.
2) A 7.98 x 10^-2 M solution of HNO3:
Similar to the previous question, we need to find the concentration of H+ ions in the solution.
Since HNO3 is a strong acid, it dissociates completely in water to give H+ and NO3- ions.
Thus, the concentration of H+ ions is equal to the concentration of HNO3, which is 7.98 x 10^-2M.
Using the equation pH = -log[H+], we can find the pH: pH = -log(7.98 x 10^-2) = 1.1.
3) 1098L of a solution containing 8.543 moles of HBr:
To find the pH, we need to know the concentration of H+ ions in the solution.
First, we need to calculate the molarity (M) of the solution by dividing the moles of HBr by the volume in liters:
Molarity (M) = moles of solute / volume of solution in liters
M = 8.543 moles / 1098 L ≈ 0.0078 M
Since HBr is also a strong acid, it dissociates completely in water to give H+ and Br- ions.
Thus, the concentration of H+ ions in the solution is 0.0078 M.
Using the equation pH = -log[H+], we can find the pH: pH = -log(0.0078) = 2.1.
4) 120 mL of a solution containing 0.005 grams of hydrochloric acid:
To find the pH, we need to calculate the molarity of the solution.
First, we need to convert the mass of HCl from grams to moles using its molar mass, which is 36.46 g/mol:
moles of HCl = mass / molar mass
moles of HCl = 0.005 g / 36.46 g/mol ≈ 0.000137 mol
Next, we need to calculate the molarity (M) of the solution by dividing the moles of HCl by the volume in liters:
Molarity (M) = moles of solute / volume of solution in liters
M = 0.000137 mol / 0.120 L ≈ 0.00114 M
Since HCl is also a strong acid, it dissociates completely in water to give H+ and Cl- ions.
Thus, the concentration of H+ ions in the solution is 0.00114 M.
Using the equation pH = -log[H+], we can find the pH: pH = -log(0.00114) = 2.94.
Answering your second question, having only four questions you don't understand out of 20 is actually pretty good! It shows that you understand the majority of the material. Keep up the good work! If you have any more questions, feel free to ask.