In a titration of 16.0 mL of a 0.526 M solution of a diprotic acid H₂CH₂O (fumaric acid) with 0.137 M KOH, how many mL of base are required to reach the second equivalence point?

The acid HX has a pKa of 5.00.  If 25.00 mL of a 0.106 M solution of HX are titrated with 0.100 M NaOH solution, what's the pH after 11.28 mL ofbase solution is added?

In a titration of 25.0 mL of 0.10 M phosphoric acid (a triprotic weak acid) with 0.20 M NaOH, what species are present after the addition of 20.0 mL of NaOH?What species would be present if we only added 10 mL NaOH?

In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is the pH calculated before the titrant is added? Group of answer choices The pH is based on the concentration of protons present in the solution, which is equal to the original concentration of the acid. The pH is calculated using the H-H equation for a buffer solution, using the ratio of the concentrations of the base and the acid, and the pKa of the acid. The pH is 7. The pH is calculated by determining the concentration of weak conjugate base present in the solution, using an ICE table to calculate the hydroxide ion concentration present after hydrolysis, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of weak acid present in the solution, using an ICE table to calculate…

A certain weak acid, HAHA, with a KaKaK_a value of 5.61×10−65.61×10−6, is titrated with NaOHNaOH. A solution is made by titrating 8.00 mmolmmol (millimoles) of HAHA and 1.00 mmolmmol of the strong base. What is the resulting pH?   More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 47.0 mL ?

You need to prepare an acetate buffer of pH 5.455.45 from a 0.843 M0.843 M acetic acid solution and a 2.06 M KOH2.06 M KOH solution. If you have 630 mL630 mL of the acetic acid solution, how many milliliters of the KOHKOH solution do you need to add to make a buffer of pH 5.455.45? The p?apKa of acetic acid is 4.76.4.76. Be sure to use appropriate significant figures.   mL

Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60   mL(b) What is the pH at the equivalence point?  5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid?  (d) What is the pH of the solution after the addition of 82.9 mL of acid?  only need part c and d please

a saturated solution of M(OH)2 is prepared. 15 ml of the saturated solution was titrated with a .055 M HCL solution. Examination of the pH titration curve indicated that it took 8.15 ml of the HCL solution to reach the equivalence point. What is the [OH-] in the saturated solution

What is the pH of an aqueous solution containing 75.0 mL of a 0.15M HNO2 solution and 45.0 mL of a .25M KNO2? What is the pH of this solution after 10.0 mL of a 0.20M solution of KOH is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)?