ntActivity do?locator-assignment-take@itakeAssignmentSessionLocator assignment-t

Question

ntActivity do?locator-assignment-take@itakeAssignmentSessionLocator assignment-tak c Search OWLv2 |Online teaching an.. Use the Refereaces to access important valors if needed for this question A buffer solution is made that is 0.410 M in HCIO and 0.410 M in KCIO If K, for HCIO is 3.50 × 10-8, what is the pH of the buffer solution? Write the net ionic equation for the reaction that occurs when 0.097 mol KOH is added to 1.00 L of the buffer solution (Use the lowest possible coefficients Omit states of matter.) Subnut Answer Retry Enlate Group 1 more group attempt remaining

Explanation / Answer

We know that;

pKa = -logKa = = -log(3.50 x10^ -8.) = 7.46

Henderson-Hasselbalch equation

pH = pKa + log[salt/acid]

    = 7.46 + log (0.410/.410)

    = 7.46 + log 1.0

    = 7.46 + 0.0

pH = 7.46

KOH = K+ OH-

HClO = H+ ClO-

HClO (aq)+OH(aq)--- > ClO (aq)+H2O(l)

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