***CHEMISTRY AQUEOUS EQUILIBRIA QUESTION***PLEASE HELP PLEASE ANSWER BOTH PART A

Question

***CHEMISTRY AQUEOUS EQUILIBRIA QUESTION***PLEASE HELP

PLEASE ANSWER BOTH PART A AND PART B!

± Titration of Strong Acid with Strong Base A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. A pH titration curve specifically monitors the pH as a function of the titrant. lations involving a titrati When conducting calculations involving a titration, the first step is to write the balanced chemical equation. Then, use the stoichiometric ratios developed from this equation to determine how many moles of each reagent are reacting

Explanation / Answer

HCl + NaOH ---------> NaCl + H2O

Since HCl & NaOH are both strong acid and base respectively, therefore

HCl(aq) ---------> H+ + Cl-

NaOH(aq) --------> Na+ + OH-

Now, moles of HCl present = molarity*volume of solution in litres = 0.2*0.1 = 0.02

Moles of NaOH added = molarity*volume of solution in litres = 0.25*0.05 = 0.0125

Thus, moles of HCl left unreacted = total moles of HCl present initially - moles of NaOH = 0.0075

Thus, Concentration of HCl left = moles/volume of solution in litres = 0.0075/0.15 = 0.05 M

Thus, pH = -log[H+] = -log[HCl] = -log(0.05) = 1.301

Now, at the point of equivalence, no HCl and no NaOH are present and the solution is neutral.

Hence the pH at equivalence will be 7

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