(a) A 25.0 mL sample of 0.175 M methylamine CH3NH2 (Kb = 1.3 x 10-5) is titrated with 0.150 M HBr. Find the initial pH at the ½ equivalence point after 5.0 mL of acid is added the pH at the equivalence point the pH after 5.0 mL acid is added after the equivalence point

A 25.0 mL sample of 0.150 M NH3 is titrated with 0.180 M HCI. Kb of NH3 = 1.76 x 10-5 Show your calculations. a) Write the neutralization reaction. b) What volume of 0.180 M HCI is required to reach the equivalence point? c) What is the pH at the equivalence point? d) Explain why the pH is not equal to 7 at the equivalence point. e) What is pH at the midpoint? f) What is the pH after 30.0 mL of 0.180 M HCI has been added. g) Draw a reasonable titration curve label the equivalence point and the midpoint. A

65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid.

Select all that are true for a titration at the equivalence point: Group of answer choices The number of moles of acid (ie H2SO4) added are the same as the number of moles of base (ie NaOH) added.   The number of moles of hydronium ion added are the same as the number of moles of hydroxide ion added. The indicator is selected in order to have a color change when the equivalence point is reached.

Find the pH of the reaction mixture after the addition of the given volume (see below for your assignment) of 0.25M hydrochloric acid to a 20.0 mL sample of .15M potassium fluoride (Ka for HF =7.2 x 10^-4) 13.5 mL HCl added Weak base, strong acid pH curve Titration, post equivalence point

A 20.0 mL sample of 1.80 M formic acid, HCHO2, is titrated with a 2.40 M NaOH solution. pKa = 3.74 for formic acid. Calculate the pH at the following points of the titration: a) After adding 5.00 mL of NaOH  b) ½ equivalence point  c) Equivalence point

Consider the titration of 40 mL of 0.2 M NH3 with 0.5 M HCI. Calculate the pH after addition of the following amounts of 0.5 M HCI at 25 °C Part A O mL (initial pH) ? νη ΑΣφ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part B 5 mL ? Πν ΑΣφ Submit Request Answer Part C half-way to equivalence point

1) You have 10 mL of a buffer that is 0.1 M acetic acid and 0.1 M sodium acetate. How many mLs of 0.025 M HCl will need to be added in order to reach a pH of 4.65? (Kafor acetic acid is 1.82 x 10-5)

You have  0.100 M  solutions of acetic acid ( p?a  =  4.76 ) and sodium acetate. If you wanted to prepare  1.00 L  of  0.100 M  acetate buffer of pH  4.00 , how many milliliters of acetic acid and sodium acetate would you add?

Bewis a titra on curve of a weak acid with NaOH. What region of the titration curve can the volume of NaOH at equivalence point be located? O с B A 2 A B Vol. NaOH (mL) 6 C 8 10