Write the net ionic equation for the reaction of potassium hydrogen phthalatc an

Question

Write the net ionic equation for the reaction of potassium hydrogen phthalatc and sodium hydroxide. In the image which figure of is depicting a basic/alkaline solution, an acidic solution, and a neutralized solution where phenolphthalcin is the indicator? Using the images below, what is the initial buret reading for the titration? What is the final reading? How much liquid was dispensed? You obtain a 0.956 g sample with an unknown amount of KHP (mol. wt. 204.22 g/mol). You then find that it takes 21.06 mL of 0.128 M NaOH to neutralize your sample. What percentage of KHP is in your unknown?

Explanation / Answer

KHC8H4O4 + NaOH -----------------> KNaC8H4O4 + H2O

I solution is basic solution

II solution is neutral solution

III solution is acidic solution

3. volume = final volume - intial volume

                  =24.3-9.7 = 14.6ml

4.

KHC8H4O4 + NaOH -----------------> KNaC8H4O4 + H2O

1 mole           1mole

no of moles of NaOH = molarity *volume in L

                                    = 0.128*0.02106 = 0.002695 moles

no of moles of KHC8H4O4 = no of moles of NaOH

no of moles of KHC8H4O4   = 0.002695 moles

mass of KHC8H4O4     = 0.002695*204.22 = 0.55g

percent mass = 0.55*100/0.956 = 57.53%

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