1.
When HNO3 (flask) is titrated with KOH (burette), which response best describes the equivalence point?
Group of answer choices
A) The pH > 7 since there is a strong base present.
B) The pH = 7 since it has the same moles of acid and base present.
C) The pH < 7 since there is a strong acid present.
D) The pH < 7 since the conjugate acid would be present.
E) The pH > 7 since the conjugate base would be present.
2.
When HCOOH (flask) is titrated with NaOH (burette), which response best describes the pH at the equivalence point?
Group of answer choices
A) The pH < 7 since the conjugate acid would be present.
B) The pH > 7 since the conjugate base would be present.
C) The pH > 7 since there is a strong base present.
D) The pH = 7 since it has the same moles of acid and base present.
E) The pH < 7 since there is a strong acid present.
1)
HNO3 is strong acid and KOH is strong base.
So, at the equivalence point, the solution would be neutral and pH
would be 7.00
Answer: B
2)
HCOOH is weak acid.
NaOH is strong base.
At equivalence point equal mol of both will react to form
HCOO-.
HCOO- is conjugate base and hence pH would be greater than 7
Answer: B
1. When HNO3 (flask) is titrated with KOH (burette), which response best describes the equivalence point?...
When HNO3 (flask) is titrated with KOH (burette), which response best describes the equivalence point? O The pH = 7 since it has the same moles of acid and base present. The pH > 7 since the conjugate base would be present. The pH <7 since the conjugate acid would be present. The pH > 7 since there is a strong base present. The pH <7 since there is a strong acid present.
How many mL of 0.233 M HNO3(aq) are needed to neutralize 56.90 mL of a 0.1368 M solution of barium hydroxide, Ba(OH)2? answer choices: 53.9 66.8 100.2 33.4 16.7 2) When HNO3 (flask) is titrated with KOH (burette), which response best describes the equivalence point? Group of answer choices The pH < 7 since there is a strong acid present. The pH = 7 since it has the same moles of acid and base present. The pH > 7 since...
Find the pH at the equivalence point of HA being titrated by BOH, where HA is a weak acid with a ka=4.3*10-4 and BOH is a strong base you have Building on problem 1, if you have 0.1 M NaOH and find your equivalence point at 23.78 mL added, how many moles of HA were present? Find the equivalence point and the pH at equivalence of .234 moles of citric acid being titrated with 0.100 M KOH. Acetic acid is...
Mark each of the following statements about the ½ equivalence point of an acid-base titration TRUE or FALSE. a. It is the point in the titration when the concentration of weak acid (HA) being titrated is equal to the concentration of the conjugate base (A− ). b. It is the point halfway between the beginning of the titration of a weak acid or weak base and the equivalence point. 2 c. When a strong acid is titrated with a strong...
1. A 30.00 mL sample of 0.400 M HNO3 is titrated with 0.600 M KOH. What is the balanced neutralization chemical reaction? What volume of base (in mL) must be added to reach the equivalence point? Is the pH of the equivalence point acidic, basic, or neutral?
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
When a weak acid is titrated with a strong base, if the pH at the half-equivalence point is 6.04, what is the Ka of the acid?
What is the pH at the equivalence point when 0.112 M hydroxyacetic acid is titrated with 0.0500 M KOH?
Equivalence Point - this is the point where the moles of the titrant are equal to the moles of titrated solution 25ml. 0.10M HNO, with 0.10M KOH 25ml 0.10M CH,COOH with 0.10M NaOH 25ml 0.10M NH, with 0.10M HCI Weak Base /Strong Acid What volume of strong acid is needed to reach the equivalence point? Determine the final concentrations (molarity) after the addition of this much acid. "Remember The total volume will have changed Moles before Change Moles after Final...
In which of the following titrations would the solution be neutral at the equivalence point? [Hint: For a neutral equivalence point, we need both a strong acid and a strong base as analyte and titrant, respectively.] HOCl titrated with Ba(OH)2 CH3COOH titrated with NaOH HClO4 titrated with KOH Sr(OH)2 titrated with H3PO4 NH3 titrated with HCl