What is the difference between the endpoint and equivalence point in a titration? Group of answer choices 1.the endpoint is when the pH is exactly 7 2.the equivalence point is when the pH is exactly 7 3.the endpoint and the equivalence point are the same thing 4.the equivalence point is where moles of OH- equals H+, while the end point is where a color change occurs.

2. In the second titration, the molar mass of an unknown monoprotic acid is calculated.  If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186

Question 6 Type numbers in the boxes. 45.0 mL of o.650 M HNO, is titrated by 0.650 M KOH. aby Part 1: 10 points Calculate the pH of the acid solution before any titrant is aby Part 2: 10 points added. aby Part 3: 1 points pH = aby Part 4: 10 points Calculate the pH after 1.47 mL of o.650 M KOH is added 31 points to 45.0 mL of 0.650 M HNO,. pH = Calculate the pH after 45.00 mL of o.650 M KOH is added to 45.0 mL of o.650 ΜΗΝΟ. pH = Calculate the pH after 89.5 mL of o.650 M KOH is added to 45.0 mL of 0.650 M HNO,- pH =

Macmillan Learning Select the statements that describe a method which can be used to make a buffer. Partially neutralize a strong acid solution by addition of a strong base. Add appropriate quantities of weak acid and its conjugate base to water. Partially neutralize a weak base solution by addition of a strong acid. Partially neutralize a strong base solution by addition of a strong acid. Partially neutralize a weak acid solution by addition of a strong base. OCT 12 3o) N A

You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.050 M HOAc and 0.050 M NaOAc.   How do the pHs of the buffered solutions compare?   Select one: a. The pH of buffered solution 1 is greater than that of buffered solution 2. b. The pH of buffered solution 2 is greater than that of buffered solution 1. c. The pH of buffered solution 1 is equal to that of buffered solution 2. d. Cannot be determined without the Ka values. e. None of these (A-D).

What is a buffer?  Choose 2.   a solution that resists changes in pH a solution that neutralizes a basic solution a weak acid-base conjugate pair a solution that neutralizes an acidic solution a strong acid-base conjugate pair

QUESTION 5 When titrating a strong monoprotic acid and KOH at 25°C, the O pH will be equal to 7 at the equivalence point. titration will require more moles of base than acid to reach the equivalence point. O pH will be less than 7 at the equivalence point. pH will be greater than 7 at the equivalence point. titration will require more moles of acid than base to reach the equivalence point.

A buffer pair consists of a conjugate weak acid0weak base pair that will resist a change in pH from the addition of a strong acid or base. Decide whether each pair below is a good example of a buffer.a. HCN and NaCN  Good Buffer or Not a Bufferb. H2CO3 and Na2CO3  Good Buffer or Not a Bufferc. H2SO4 and NaHSO4  Good Buffer or  Not a Buffer

Which of the following is not a characteristic of buffer solutions? O They cannot be tailored to maintain a specified pH. O They contain a conjugate base of a weak acid. O They contain a weak acid. O They have a finite capacity for accommodating added acid or base. O They can maintaln their pH, even when small amounts of acid or base are added. QUESTION 10 The capacity of a buffer solution is greater when there are large amounts of a weak acid and its conjugate base in solution. O True O False

1.  all the aqueous solutions that are good buffer systems 2.  a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution.  3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…