A 117.0 mL sample of 0.100 A methylamine (CH₂NH₂; K-3.7 x 10-) is strated with 0.205 M HNOS. Calculate the pit ater the addition of each of the following volumes of acid Part A Express the pH to two decimal places. pil. Submit Be Part B 22.2 ml Express the pH to two decimal places. pl Part C var Pans 22 V for Partre Submit pl 44.4 ml. Express the pH to two decimal places. Part D fog Pag 12 2018 Voo for Part redo tot refor Pan 8 keyboard shortcuts for Part help for Pan Submit pl. for Party Parto for Part redo forer Part C keyboard shortcuts for Part C help & Part 000 ml. Express the pH to two decimal places. A PA Part keyboard shortcuts for Part A her Part Submit Para o for Part&redotorer Part D keyboard shortcuts for Part D help & Part D

In a titration of 73.0 mL of a 0.500 M solution of a diprotic acid H.C.H.O. (malonic acid) with 0.255 M NaOH, how many grams of NaOH are required to reach the second equivalence point? (MW_NaOH = 39.997 g/mol) B

A solution of 0.0470 M HCl is used to titrate 26.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 16.0 mL HCl solution have been added. (Assume KW=1.01e-14). What was the pH at the equivalence point?

b) What is th 1 с E 10. If a 50.0-mL sample of 0.250 M NaCN is titrated by 0.250 M HCI (strong acid), what is the pH of the solution at the equivalence point? Ka of Hydrocyanic Acid (HCN) at 25 °C is 6.2 x10-10. Hydrocyanic acid ce reacts with water to produce hydronium and cyanate.

1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid  has a pKa of 8.27.  Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE

Calculate the pH of each of the following solutions   a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5   b. 0.10 M sodium propanoate, NaCH3CH2COO.   c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate   d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate   e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate

A 20.00 mL of 0.100 M diprotic weak acid H2A is titrated with 0.200 M NaOH. The volume of the NaOH solution required to change the pH of the solution to a value equal to the pKa1 of the acid is

Hh.129.

5. a. Suppose a solution contains 0.50 M NaH2PO4 and 0.80 M Na2HPO4. What pH should be expected for this buffer solution? Uw we made aw bufter b. Calculate the final pH if 5.0 mL of 0.10 M NAOH is added to 20.0 mL of this buffer solution. it +corected

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10-5