At the equivalence point, the following titrations (just a mixture of two solutions) give either acidic or basic solutions. mixture Type of solution Relevant K values а. NaOH + HCN basic K, of HCN = 4.9 x 10-10 b. NaOH + HNO2 basic Ka of HNO2 4.0 x 10-4 %3D c. HCI + NH3 acidic K, of NH3 = 1.8 x 10-5 %3D For each mixture, (1) write the major species present at the equivalence point, and (2) equilibrium reaction that produces the acidic or basic solution.

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

C Determine the pH of each solution at the equivalence point. pH (NaOH titrant) pH (Ca(OH)2 titrant) Submit =

2)Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points and tell how many milliliters of acid are required to reach the equivalence point. a)Before the titration starts b)At the equivalence point c)After an additional 10.0 mL of HCL is added after the equivalence point (i.e. equivalence point volume + 10.0 mL)

I need help with 3. Determine the pH of the solution at the equivalence point

In a titration of a weak acid with a strong base, what is the pH of the solution at the equivalence point?

se or conjugate base. 12 2. A 50.0mL sample of an acid HA, of unknown molarity is titrated with 0.1000 M KOH. The pH of the resulting solution is measure with a pH meter and graphed below. Select the letter that corresponds to the following. Some letters may be used more than once. Some may not be used at all. 10+ a. the equivalence point: R 9 b. the half equivalence point: Q 8+ c. where [KOH] is greatest: 7+ P I of d. where [H+] is greatest: T e. where [HA]=[A-]: 5+ 4 f. where [A-] is the predominate species: 3+ 2 SO a. What is pH after 10.0mL of 0.15M NaOH solution has been added to 25.0 mL of 0.12M HF solution? Ka = 6.8 x 10-4. b. After adding NaOH, is the resulting solution a buffer solution? Explain. 3. Complete the following calculations. (P) (Q) 84 3 ST PR

A triprotic acid is titrated with KOH. What species are NOT in solution to any large extent between the 1st and 2nd equivalence points? Select all that apply. O H3A O HA? O A³- K+ O OH H2A

HCN is a weak acid with a Ka = 4.90 x 10-10. A 50.00 mL sample of this HCN solution (0.250 M) is titrated with 0.500 M NAOH. What is the pH at the equivalence point?

Let HA represent a weak acid. A 10.0 mL sample of 0.600M HA was titrated with 0.300 M NaOH. The table below is some of the data for this titration. Volume NaOH added (mL) 5.00 10.00 15.00 ? ? pH 6.98 7.46 7.93 ? ? Calculate the following: a) The volume of NaOH needed to reach the equivalence point is mL. (Report value to the correct number of significant figures.) b) The Ka for HA is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) c) The Kp for A is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) d) The pH of the solution at the equivalence point is e) On your sheet of paper, draw a reasonable diagram of the complete titration curve. Label both axis appropriately. Label the volumes and pH values at the MIDPOINT and the EQUIVALENCE POINT.