Respuesta :
Answer:
A. [H₃O⁺] = 0.900 M
B. pH = 0.0 to one decimal place
C. [H₃O⁺] = 0.620 M
D. pH = 0.21 to two decimal places
Explanation:
A. Equation for the complete dissociation of H₃PO₄ is given below:
H₃PO₄(s) + 3H₂O(l) -----> PO₄³⁻(aq) + 3H₃O⁺(aq)
From the equation of reaction, one mole of H₃PO₄ produces 3 moles of H₃O⁺
Therefore, [H₃O⁺] = 3 * 0.300M = 0.900 M
B. pH = -log[H₃O⁺]
pH = - log(0.900)
pH = -log (9 * 10⁻¹)
pH = 0.0 to one decimal place
C. Equation for the complete dissociation of H₂C₂O₄ is given below:
H₂C₂O₄(s) + 2H₂O(l) ----> C₂O₄⁻(aq) + 2H₃O⁺
From the equation of reaction, one mole of H₂C₂O₄ produces 3 moles of H₃O⁺
Therefore, [H₃O⁺] = 2 * 0.310 M = 0.620 M
D. pH = -log[H₃O⁺]
pH = -log(0.620)
pH = -log(0.62 * 10⁻¹)
pH = 0.21 to two decimal places
The concentration of [[tex]\rm H_3O^+[/tex]] has been 0.9 M, and the pH has been 0.045.
The polyprotic acid has been able to donate more than one proton in an acid-base reaction.
The balanced chemical reaction can be:
[tex]\rm H_3PO_4\;+\;3\;H_2O\;\rightarrow\;PO_4^3^-\;+\;3\;H_3O^+[/tex]
(a) According to the equation, 1 mole of [tex]\rm H_3PO_4[/tex] gives 3 moles of hydronium ions. The molarity has been defined as moles per liter. Assuming the volume of reaction to be 1 liter.
1 mole [tex]\rm H_3PO_4[/tex] = 1 M [tex]\rm H_3PO_4[/tex]
1 mole [tex]\rm H_3PO_4[/tex] = 3 moles [[tex]\rm H_3O^+[/tex]]
0.3 mole [tex]\rm H_3PO_4[/tex] = 3 [tex]\times[/tex] 0.3 moles [[tex]\rm H_3O^+[/tex]].
0.3 mole [tex]\rm H_3PO_4[/tex] = 0.9 moles [[tex]\rm H_3O^+[/tex]]
The concentration of [[tex]\rm H_3O^+[/tex]] has been 0.9 mole/L, or 0.9 M.
(b) pH of the solution can be defined as:
pH = -log [[tex]\rm H_3O^+[/tex]]
pH = -log (0.9)
pH = 0.045
The pH of the solution has been 0.045.
(c) The polyprotic acid have the balanced equation:
[tex]\rm H_2C_2O_4\;+\;2\;H_2O\;\rightarrow\;C_2O_4^-\;+\;2\;H_3O^+[/tex]
According to the equation, 1 M [tex]\rm H_2C_2O_4[/tex] gives 2 M [tex]\rm H_3O^+[/tex].
The concentration of hydronium ions from 0.310 M [tex]\rm H_2C_2O_4[/tex] has been:
1 M [tex]\rm H_2C_2O_4[/tex] = 3 M [tex]\rm H_3O^+[/tex]
0.310 M [tex]\rm H_2C_2O_4[/tex] = 2 [tex]\times[/tex] 0.310 moles [[tex]\rm H_3O^+[/tex]]
0.310 M [tex]\rm H_2C_2O_4[/tex] = 0.62 M [[tex]\rm H_3O^+[/tex]].
The [[tex]\rm H_3O^+[/tex]] concentration of the solution has been 0.62 M.
(d) pH of the solution can be defined as:
pH = -log [[tex]\rm H_3O^+[/tex]]
pH = -log (0.62)
pH = 0.20
The pH of the solution has been 0.20.
For more information about the pH of the solution, refer to the link:
https://brainly.com/question/1265333
