In Test 1 you will carry out a titration between the solution of your product (which is basic) and the solution of HCl (which is acidic). To carry out a reasonable titration you will want to use about 10-20 mL of the HCl. The concentration of the HCl(aq) you'll be using is 1.00 M. 11. If the titration requires 11.52 mL of 1.00 M HCl, how many moles of HCl is this

Phosphoric acid is a triprotic acid ( =6.9×10−3 , =6.2×10−8 , and =4.8×10−13 ). to find the ph of a buffer composed of h2po−4(aq) and hpo2−4(aq) , which p value should be used in the henderson–hasselbalch equation? p k a1 = 2.16 p k a2 = 7.21 p k a3 = 12.32 calculate the ph of a buffer solution obtained by dissolving 18.0 18.0 g of kh2po4(s) kh 2 po 4 ( s ) and 33.0 33.0 g of na2hpo4(s) na 2 hpo 4 ( s ) in water and then diluting to 1.00 l.