A(OH)3 (s) ⇒ A³+ (aq) + 3OH¯(aq) When a 10.0 mL sample of a saturated solution of this salt was titrated, it required 2.03x10-3 mol HCI to reach the endpoint. Determine the Ksp value for the unknown. a) 6.29x10-13 hydroxide has the following solubility reaction: Ob) 5.09x10-1 -13 Oc) 5.66x10-12 d).5.66x10-20

12 a b U Consider a buffer made by adding 132.8 g of NaC,H,O₂ to 300.0 mL of 1.83 M HC,H,O₂ (Ka = 6.3 x 10-5) X L L What is the pH of this buffer? What is the pH of the buffer after 0.750 mol of H+ have been added? What is the pH of the buffer after 0.250 mol of OH- have been added? >

When a 16.4 mL sample of a 0.368 M aqueous hydrocyanic acid solution is titrated with a 0.332 M aqueous barium hydroxide solution, what is the pH after 13.6 mL of barium hydroxide have been added? pH = 1

-3 A chemistry graduate student is given 450. mL of a 1.10M diethylamine ((C₂H), NH) solution. Diethylamine is a weak base with K₂ = 1.3 × 10¯ What mass of (C₂H₂)2NH₂Cl should the student dissolve in the (C₂H5) NH solution to turn it into a buffer with pH = 11.25? You may assume that the volume of the solution doesn't change when the (C₂H5) NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 Explanation 85°F Mostly sunny Check $ D x10 X C % S E F6 Q Search. F7 & L FB a * F9 F10 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi *- F11 *+ F12 PrtSc Insert Delete 4)

A 52.0-mLmL volume of 0.35 MM CH3COOHCH3COOH (Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 MM NaOHNaOH. Calculate the pHpH after the addition of 21.0 mLmL of NaOHNaOH.

A buffer solution is prepared in such a way that the concentration of propanoic acid is 3.9 x 10-1 power M and the concentration of sodium propanoate is 1.8 x 10 0 power M.  The buffer equilibrium is described by C2H5cooH + H20 both arrows H3O+ c2h5COO-    with Ka= 1.34 x 10 - 5 power . if the concentration of the sodium propanoate were double propanotate were doubled while the acide concentration remained the same, calculate the pH of the resulting solution  pH = _______