Calculate the PH concentrated hydrochloric acid if this solution is 24.8% HCL by weight and has a density of 1.16g/ml. I do not understand the right answer 0.90PH Why? Please help
My calculation
1.18g/ml x 1000ml x 0.248/36.5 = 7.8M
I cannot do?
I think your 7.8 is ok if you carried it out one more place. I obtained 7.88. Then pH = -log(H^+) = -log(7.88) = 0.8966 which rounds to 0.90 to two s.f.
A solution of sodium cyamide nacn has a ph of 12.10. How many grams of nacn are in 425ml of solution with the same PH
Who helps me to solve it for me. Step by step
To calculate the pH of a concentrated hydrochloric acid solution, you will need to consider the concentration of HCl and the density of the solution. Here's how you can determine the correct answer:
1. Calculate the molarity (M) of the hydrochloric acid solution:
- Convert the density of the solution from g/ml to g/L:
1.16 g/ml x 1000 ml/L = 1160 g/L
- Calculate the mass of HCl in the solution:
1160 g/L x 0.248 = 287.68 g/L
- Calculate the molarity of HCl using the molar mass of HCl:
M = (mass of solute in grams) / (molar mass in g/mol)
M = 287.68 g/L / 36.5 g/mol ≈ 7.88 M
2. Convert the molarity to the hydrogen ion concentration ([H+]):
- For hydrochloric acid (HCl), the concentration of H+ ions in the solution will be the same as the HCl concentration.
- [H+] = 7.88 M
3. Calculate the pH using the equation:
pH = -log[H+]
pH = -log(7.88)
pH ≈ 0.90
Therefore, the correct answer is approximately pH 0.90 for the concentrated hydrochloric acid solution. Your calculated result of 7.8 M is correct, but you made a mistake in converting the molarity to pH by not using the "-log" function. The correct calculation for pH is -log(7.8), which gives a result of approximately 0.90 pH.