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lana [24]
3 years ago
7

Select all of the statements that are true about a buffer solution. Select one or more: a. A buffer solution reacts with basic s

olutions. b. A buffer solution has a pH of 7. c. A buffer solution reacts with acidic solutions. d. A buffer solution always changes color when the pH changes. e. A buffer solution resists small changes in pH. Question 13 Not yet answered Marked out of 1.00 Not flaggedFlag question Question text At what point on the titration curve for a weak acid is the solution a buffer

Chemistry
1 answer:
zhuklara [117]3 years ago
5 0

Answer:

a. A buffer solution reacts with basic solutions.

c. A buffer solution reacts with acidic solutions.

e. A buffer solution resists small changes in pH

Explanation:

1. Buffer questions

a, c, and e are TRUE. A buffer resists a change in the pH when small amounts of a strong acid or base are added to it.

b is wrong. A buffer can have a pH of 7, but it can also have many other pH values.

d is wrong. Most buffers are colourless, and they resist a change in pH.

2. Titration curves

The solution is the best buffer at the mid-point of the titration curve.

In the figure below, the equivalence point is at 13 mL, so the mid-point is at 6.5 mL.  

The solution is buffered at pH 3.2.

However, the solution is a buffer at any point in the range pH = 3.2 ± 1.

That would be in the range of 1 mL to 12 mL.

The buffering ability becomes worse the further you are from the mid-point of the titration.

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Darya [45]

Answer:

See Explanation

Explanation:

The equation of the reaction;

KHSO4(aq) + KOH(aq) -------> K2SO4(aq) + H2O(l)

Number of moles of KHSO4 = 49.6 g/136.169 g/mol = 0.36 moles

Since the reaction is in a mole ratio of 1:1, 0.36 moles of K2SO4 is produced.

Number of moles of KOH = 25.3 g/56.1056 g/mol = 0.45 moles

Since the reaction is 1:1, 0.45 moles of K2SO4 is produced

Hence K2SO4 is the limiting reactant.

Mass of K2SO4 formed = 0.36 moles of K2SO4 * 174.26 g/mol = 62.7 g

So;

1 mole of KHSO4 reacts with 1 mole of KOH

0.36 moles of KHSO4 reacts with 0.36 * 1/1 = 0.36 moles of KOH

Amount of excess KOH = 0.45 moles - 0.36 moles = 0.09 moles

Mass of excess KOH = 0.09 moles * 56.1056 g/mol  = 5 g of excess KOH

5 0
3 years ago
What mass in grams of Ag is produced from reaction of 31.75 g of Cu
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<span>Copper metal (Cu) reacts with silver nitrate (AgNO3) in aqueous solution to form Ag and Cu(NO3)2. An excess of AgNO3 is present. The balanced chemical equation is shown below.

Cu + 2AgNO3 ---> Cu(NO3)2 + 2Ag

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