Question

Compared with a basic solution of pH12 the same volume of an acidic
solution at pH 4 has how many times more hydrogen ions. Show how
you derived this figure .

Can you explain it step by step thx :)

Answer #1

See we know that

pH= -log[H+] (base 10)

First find the concentrations of [H+] using the pH values given in the question. And then take the ratio of the two [H+] concentrations to find out how many times more hydrogen ions corresponds to pH 4.

so if pH is 12,

12 = -log[H+]

[H+] = antilog[-12]

**[H+] = 1 x 10^-12 -(1)**

Similarly find the concenration of [H+] for pH = 4

4 = -log[H+]'

[H+]' = antilog[-4]

**[H+]' = 1 x 10^-4 -(2)**

**divide (1) by (2)**

**[H+]' / [H+] = 1 x 10^-4 / 1 x 10^-12**

**[H+]' = 10^8 [H+]**

So the concentration of [H+] ions at pH 4 is 10^8 times more than the concentration of [H+] at pH 12.

This peptide, Lys-Glu-Ala-Asp-Arg-Met-Arg, will be isoelectric
at what pH range?
A. neutral
b. acidic
c. basic
d. very basic
The answer is C. Can you please explain how to figure this
out.

How does a solution of pH 7 compare to a solution of pH 10?
pH 7 has more OH- ions
pH 7 is more basic
pH 7 has a higher pH
pH 7 has more H+ ions
When working with acids, which of the following is the proper
way to dilute these chemicals?
Add water to the acid in a beaker.
Add the acid to water.
Place acid in a graduated cylinder then add water to the correct
volume.
None...

Determine whether each of the following will form a solution
that is acidic, basic, or pH-neutral.
1) Fe(NO3)3
2) KCl
3) K2CO3
4)CH3NH3Cl
5) C2H5NH3CN

Determine the pH of water solutions with the following
characteristics. Classify each solution as acidic, basic, or
neutral.
(a) [OH negative]=9.4 *10 to the negative 4 power
(b) [OH negative]=10.[H positive]
(c) [H positive]=2.3 * 10 to the negative 2 power
(d) [OH negative]=5.1 * 10 to the negative 10 power
Please show work in obvious steps and clear handwriting. Thank
you so much!

A solution with a pH of 10
a. Has a hydrogen ion concentration [H+ ] of 10^10 M
b. Has a hydroxide ion concentration [OH] of 10^4 M
c. Has twice as many H+ s as a solution at pH 8
d. Has 10× as many H+ s as a solution at pH 11
can you please explain how you could find the answer?

18. Which H3O+ concentration and classification (acidic vs.
basic) are correctly matched for a solution in which the OH-
concentration is 5.6 x 10-6 M?
a. 5.6 x 10-6 M : basic
b. 5.6 x 10-6 M : acidic
c. 5.6 x 108 M : acidic
d. 1.8 x 10-9 M : basic
e. 1.8 x 10-9 M : acidic
19. The solution that will give a pH = 12.00 is (MW: NaOH = 40
g/mol):
a. 4.0 g NaOH...

pH
4 is how many times more acidic than pH10?
a. 6 times
b. 610 times
c. 106 times
d. 600 times
e. 60 times

Complete the following table:
H3O+
OH−
pH
Acidic, Basic, or Neutral?
10.0
Neutral
4×10−5M
1 ×10−2M
12.2
Part A
If the pH of the solution is 10.0, what is the [H3O+]?
Express your answer to one significant figure.
[H3O+] =
M
Part B
If the pH of the solution is 10.0, what is the [OH−]?
Express your answer to one significant figure.
[OH−] =
M
Part C
If the solution is neutral, what is the [H3O+]?
Express your answer to...

which pairs the first compound more acidic
HCL02 or HBr02
and can you explain how you can figure it out
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consider the oxidation of iron2 to iron3 by hydrogen peroxide in
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Please explain how you get N in the equation as well, cant seem
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