1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
gulaghasi [49]
3 years ago
8

Equal volumes of two monoprotic acid solutions (A and B) are titrated with identical NaOH solutions. The volume to reach the equ

ivalence point for solution A is twice the volume required to reach the equivalence point for solution B, and the pH at the equivalence point of solution A is higher than the pH at the equivalence point for solution B. Which statement is true?
A) The acid in solution A is less concentrated than in solution B and is also a weaker acid than that in solution B.
B) The acid in solution A is more concentrated than in solution B and is also a stronger acid than that in solution B.
C) The acid in solution A is less concentrated than in solution B and is also a stronger acid than that in solution B.
D) The acid in solution A is more concentrated than in solution B and is also a weaker acid than that in solution B.
Chemistry
2 answers:
Firlakuza [10]3 years ago
5 0

Answer:

D

Explanation:

It looks like two things are being looked at here; the concentration and strength of acid. Titrations show volume and are not affected by the strength of the acid, so let's start with that. Since twice the volume of NaOH is needed to reach equivalence point, there must be a higher concentration of A, as the chemical equation must be the same (it says that they're both monoprotic acids, so the chemical equation doesn't change). This eliminates A and C.

As for pH; if it is higher at equivalence point, it wasn't as strong at moving the pH down despite being in NaOH(a strong base); and since solution A has a higher pH at equivalence point, it isn't as strong as solution B.

This eliminates B.

The answer is D.

This seems like a normal AP Chemistry question, but then again titrations are important to know in chemistry.

agasfer [191]3 years ago
4 0

Answer:

D. Solution A has more concentrated acid than solution B and acid in solution A is also a weaker acid than that in solution B.

Explanation:

As it has been said in the question that the volume to reach the equivalence point of the solution A is twice the volume of solution B, this is because the acid in the solution A is more concentrated than B that's why more NaOH was required to reach to the equivalence point.

Since the pH at the equivalence point was greater for solution A that means the acid in solution A was a weak acid that's why the pH raised more as the NaOH was added to the solution.

You might be interested in
What is the balanced chemical equation for the reaction of potassium with sulfur?
Aneli [31]

K + S = K2S

Potassium reacts with sulfur to produce potassium sulfide

8 0
3 years ago
On the diagram above, trace the path of a light ray through these materials
makvit [3.9K]
We need the diagram to answer the question
4 0
3 years ago
8. A sample of sulfur has a mass of 223 g. How many moles of sulfur are in the sample?
Rama09 [41]

Answer:

7 moles

Explanation:

1mole of sulfur=32

x=223

=6.9

=7moles

8 0
3 years ago
Every cell is surrounded by a thin membrane. What is the main function of this cell membrane?
zubka84 [21]

Answer:

The main function of the cell membrane is to protect the cell from the outer environment.

8 0
3 years ago
Read 2 more answers
A buffer is prepared by adding 139 mL of 0.39 M NH3 to 169 mL of 0.19 M NH4NO3. What is the pH of the final solution? (Assume th
Paha777 [63]

Answer:

pH = 9.48

Explanation:

We have first to realize that NH₃ is a weak base:

NH₃ + H₂O ⇔ NH₄⁺ + OH⁻     Kb = 1.8 x 10⁻⁵

and we are adding this weak base to a solution of NH₄NO₃ which being a salt dissociates 100 % in water.

Effectively what we have here is a buffer of a weak base and its conjugate acid. Therefore, we need the Henderson-Hasselbach formula for weak bases given by:

pOH = pKb + log ( [ conjugate acid ] / [  weak base ]

mol NH₃ = 0.139 L x 0.39 M = 0.054 mol

mol NH₄⁺ = 0.169 L x 0.19 M = 0.032 mol

Now we have all the information required to calculate the pOH ( Note that we dont have to calculate the concentrations since in the formula they are a ratio and the volume will cancel out)

pOH = -log(1.8 x 10⁻⁵) + log ( 0.032/0.054) = 4.52

pOH + pH = 14 ⇒ pH = 14 - 4.52 = 9.48

The solution is basic which agrees  with NH₃ being  a weak base.

5 0
3 years ago
Other questions:
  • Converting carbon to nitrogen by increasing the number of protons from 6 to 7 and decreasing the number of neutrons from 8 to 7
    12·2 answers
  • Identify the true statements regarding α-1, 6 linkages in glycogen.A. The number of sites for enzymes action on a glycogen molec
    10·1 answer
  • A volume of 75.0 mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water. I
    9·1 answer
  • It’s a organic chemistry
    7·1 answer
  • 2 H2 + O2 → 2 H2O What is the product of this chemical reaction
    13·1 answer
  • Which best describes a chemical reaction that follows the law of conservation of matter?
    13·1 answer
  • What are 10 household items that use em waves
    8·1 answer
  • Hydrogen bonding is present in all of the following molecular solids EXCEPT ____.a) H2O2 b) PH3 c) H2SO4 d) NH3
    9·2 answers
  • can someone answer! please don't answer for points or if you don't know it and don't answer if you are guessing make sure you un
    9·2 answers
  • Fill in the blanks to complete each statement about the heating of Earth's surface.
    8·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!