Respuesta :
Answer:
0.323
Explanation:
number of moles of Ca(OH)2(s) = mass given / molar mass = 0.350 g / 74.093 g/mol = 0.00472 mol
number of mole of HNO3 = Molarity × volume in Liters = 1.0 × (45 / 1000) = 0.045 M
Ca(OH)2(s) + 2 HNO3(aq) → Ca(NO₃)₂(aq) + 2 H₂O(I)
1 mole of calcium hydroxide react with 2 mole of trioxonitrate(V)
0.00472 mole will require 0.00945 mole
but we have 0.045 mole of the acid
net mole = 0.045 - 0.00945 = 0.0356 mole
Molarity of the net mole = 0.0356 / (75/1000) = 0.475 M
pH = - log (0.475) = 0.323
The pH of the final solution is 0.323
Calculation for number of moles:
[tex]\text{ Number of moles of } Ca(OH)_2(s) = \frac{\text{Given mass}}{\text{Molar mass} }\\\\\text{ Number of moles of } Ca(OH)_2(s) = \frac{0.350g}{74.093g/mol}\\\\\text{ Number of moles of } Ca(OH)_2(s) = 0.00472 mol[/tex]
Number of mole of HNO₃ = Molarity × volume in Liters
Number of mole of HNO₃= [tex]1.0 * (45 / 1000) = 0.045 M[/tex]
From the chemical reaction:
Ca(OH)₂(s) + 2 HNO3(aq) → Ca(NO₃)₂(aq) + 2 H₂O(I)
1 mole of calcium hydroxide react with 2 mole of trioxonitrate(V)
0.00472 mole will require 0.00945 mole
There are 0.045 mole of the acid
Thus, Net mole = 0.045 - 0.00945 = 0.0356 mole
Molarity of the net mole = [tex]0.0356 * (75/1000) = 0.475 M[/tex]
Calculation of pH:
[tex]pH = - log (0.475)\\\\ pH= 0.323[/tex]
Thus, the pH of the final solution is 0.323.
Find more information about Molarity here:
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