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Nat2105 [25]
3 years ago
9

What is the ph of a 0.006 m koh solution? 1. 11.78 2. 7.00 3. 2.22 4. 8.88 5. 5.12?

Chemistry
1 answer:
Stels [109]3 years ago
4 0
The concentration of OH⁻ is first converted to pOH bu using followinf formula,

                                           pOH  =  -log [OH⁻]
Putting value,
                                           pOH  =  -log (0.006)

                                           pOH  =  2.221
As we know,
                                   pH + pOH  =  14
Solving for pH,
                                   pH  =  14 - pOH
Putting value of pOH,
                                   pH  =  14 - 2.221

                                   pH  =  11.779
Result:
           Option-1
is the correct answer.
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Mark me brainliest

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3 years ago
A lab group of students is trying to determine whether a base qualifies as an Arrhenius base or a Bronsted-Lowry base. Which stu
kolbaska11 [484]

Answer:

Student 4, because a Brønsted-Lowry base always accepts a proton from an acid to form a conjugate acid.  

Explanation:

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Student 2 is wrong. All bases will neutralize acids. That doesn't tell you the type of base.

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8 0
3 years ago
What is the concentration of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?
ss7ja [257]

Answer:

0.15 M KCl

Explanation:

(Step 1)

Convert the original volume from mL to L. Calculate the moles of the original solution.

75.0 mL / 1,000 = 0.0750 L

Molarity = moles / volume (L)

0.200 M = moles / 0.0750 L

0.0150 = moles

(Step 2)

Convert the final volume from mL to L. Calculate the final molarity.

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Molarity = moles / volume (L)

Molarity = 0.0150 moles / 0.100 L

Molarity = 0.15 M

6 0
2 years ago
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