The pH of an acidic solution is 5.59. What is [H+]?
1 answer:
Answer:
[H⁺] = 2.57x10⁻⁶ M
Explanation:
This problem can be solved using the definition of pH:
pH = -log[H⁺]
Now we <u>isolate [H⁺] in the equation</u>:
-pH = log[H⁺]
=[H⁺]
As we are given the pH by the problem, we can now proceed to calculate the [H⁺]:
[H⁺] =
[H⁺] = 2.57x10⁻⁶ M
Thus, when the pH of a solution is 5,59; the molar concentration of H⁺ species is 2.57x10⁻⁶.
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Answer:
1.30464 grams of glucose was present in 100.0 mL of final solution.
Explanation:
Moles of glucose =
Volume of the solution = 100 mL = 0.1 L (1 mL = 0.001 L)
Molarity of the solution =
A 30.0 mL sample of above glucose solution was diluted to 0.500 L:
Molarity of the solution before dilution =
Volume of the solution taken =
Molarity of the solution after dilution =
Volume of the solution after dilution=
Mass glucose are in 100.0 mL of the 0.07248 mol/L glucose solution:
Volume of solution = 100.0 mL = 0.1 L
Moles of glucose =
Mass of 0.007248 moles of glucose :
0.007248 mol × 180 g/mol = 1.30464 grams
1.30464 grams of glucose was present in 100.0 mL of final solution.