Questions LLC
Login
or
Sign Up
Ask a New Question
Science
Chemistry
Would a solution that contains a mixture of NCl and HCl be an effective buffer? Explain
1 answer
No. A buffer is made by mixing a weak acid and its conjugate base. For example, HC2H3O2 + NaC2H3O2
You can
ask a new question
or
answer this question
.
Similar Questions
Explain why a mixture formed by mixing 100 mL of 0.100M CH3COOH and 50 mL of 0.100M NaOH will act as a buffer? in adittion to
Top answer:
NaOH is a strong base; it reacts with CH3COOH, a weak acid, as follows: CH3COOH + NaOH ==> CH3COONa
Read more.
50.0 mL of 0.185M Sr(OH)2 is reacted with 35.0 mL of a solution containing 0.120g of HCl. Calculate the pOH resulting from the
Top answer:
......................Sr(OH)2 + 2HCl ==> SrCl2 + 2H2O millimoles Sr(OH)2 = mL x M = 50.0 x 0.185 =
Read more.
A buffer contains 5.00 M acetic acid and 5.00 M acetate anion. Gaseous HCl (0.010 mole) is added to 1.00 L of this buffer
Top answer:
Use the Henderson-Hasselbalch equation for part 1. For th second part, HCl will cause an increase in
Read more.
If you add 5.0 mL of 0.50 M HCl solution to 20.0 mL to Buffer C, what is the pH of the buffer? (where buffer C is 8.203 g sodium
Top answer:
mols NaAc = 8.203/60 = about 0.14 but you need to be more accurate. M NaAc = 0.14/0.1L = about 1.4M
Read more.
suppose you made a buffer solution that was 0.050M in both HC2H3O2 and NaC2H3O2.Would the pH changes resulting from the addition
Top answer:
How can we answer this without knowing what you did in the experiment and the results?
Read more.
You need to prepare 1.0 L of a buffer with a pH of 9.15. The concentration of the acid in the buffer needs to be 0.100 M. You
Top answer:
I would google "pKa table acids/bases" (without the parentheses) and look for pKa values in the 9.15
Read more.
A buffer solution is prepared by mixing 2.50 mL of 2.00M sodium acetate with 3.30mL of 0.500M HCl and diluting the buffer with
Top answer:
acetate = Ac acetic acid = HAc ------------------------- millimols Ac = mL x M = 5.00 mmols HCl =
Read more.
Adding 10.0 mL of 0.500 M HCl to 100.0 mL of pH = 7 water produces a solution with a pH of 1.34. What is the pH of the resulting
Top answer:
millimols CH3COOH = 100 millimols CH3COO- = 100 millimols HCl = 0.5M x 10 mL = 5 mn.
Read more.
Explain why a buffer made of equal concentrations of HF and F- does not change in pH when a small amount of HCl (a strong acid)
Top answer:
Buffers work because of the way they are constructed. Buffers consist of a weak acid and a salt of
Read more.
Explain why a buffer made of equal concentrations of HF and F- does not change in pH when a small amount of HCl (a strong acid)
Top answer:
In order to explain why a buffer made of equal concentrations of HF (hydrofluoric acid) and F-
Read more.
Related Questions
If you add 5.0 mL of 0.50 M NaOH solution to 20.0 mL to Buffer C, what is the change in pH of
the buffer? (where buffer C is
A buffer solution is prepared by combining 100 mL of 0.010 M HCOOH and 80 mL of 0.010 M NaHCOO.
Calculate the pH of this buffer
1. A solution is prepared such that it is 0.45 M in formic acid and 0.35 M in sodium formate.
a) Where is this mixture located on
A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that
A 120.0 mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br, What mass of HCl could this buffer neutralize before the pH
What is the pH of the buffer system after the addition of 0.10 mole of gaseous HCl to 1 L of the solution. With a buffer system
You prepare a buffer solution by dissolving 2.00 g each of benzoic acid, C6H5COOH, and
sodium benzoate, NaC6H5COO, in 750.0 mL
Which of the following pairs can be used to prepare a buffer? (select all that can apply)
a. HCl/NaCl b. HF/KF c. NH3/NH4Cl d.
Calculate the pH of the 0.20 M NH3/0.25 M NH4Cl buffer.
I calculated the pH to be 9.15 What is the pH of the buffer after the
Calculate the change in PH when 6 ml of 0.1 M HCl is added to 100 ml of a buffer solution that is 0.1 M in NH3 and 0.1 M in