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topjm [15]
2 years ago
11

BRAINLIEST!! PLZ HELP

Chemistry
1 answer:
cluponka [151]2 years ago
4 0

Answer:

1.0 is Answer

Explanation:

May be this is helpful!

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Ionic compounds are normally in which physical state at room temperature?
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Some safety precautions people should take when using fireworks
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Answer:

Do not try to re-light or handle malfunctioning fireworks. Soak both spent and unused fireworks in water for a few hours before discarding.

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3 years ago
A substance has an atomic number of 80 and a mass number of 178. How many protons does this atom have? How many neutrons does it
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2 years ago
Do parts a, b and c
Leona [35]

Answer:- (a)The pH of the buffer solution is 3.90.

(b) the pH of the solution after addition of HCl would be 3.60.

(c) the pH of the buffer solution after addition of NaOH is 4.32.

Solution:- (a) It is a buffer solution so the pH could easily be calculated using Handerson equation:

pH=Pka+log(\frac{base}{acid})

pKa can be calculated from given Ka value as:

pKa=-logKa

pKa=-log(6.3*10^-^5)

pKa = 4.20

let's plug in the values in the Handerson equation:

pH=4.20+log(\frac{0.025}{0.05})

pH = 4.20 - 0.30

pH = 3.90

The pH of the buffer solution is 3.90.

(b) Let's say the acid is represented by HA and the base is represented by A^- .

Original mili moles of HA from part a = 0.05(100) = 5

original mili moles of A^- from part a = 0.025(100) = 2.5

mili moles of HCl that is H^+ added = 0.100(10.0) = 1

This HCl reacts with the base present in the buffer to make HA as:

A^-+H^+\rightarrow HA

Total mili moles of HA after addition of HCl = 5+1 = 6

mili moles of base after addition of HCl = 2.5-1 = 1.5

Let's plug in the values in the Handerson equation again. Here, we could use the mili moles to calculate the pH. The answer remains same even if we use the concentrations also as the final volume is same both for acid and base.

pH=4.20+log(\frac{1.5}{6})

pH = 4.20 - 0.60

pH = 3.60

So, the pH of the solution after addition of HCl would be 3.60.

(c) mili moles of NaOH or OH^- added to the original buffer = 0.05(15.0) = 0.75

This OH^- reacts with HA to form A^- as:

HA+OH^-\rightarrow H_2O+A^-

mili moles of HA after addition of NaOH = 5-0.75 = 4.25

mili moles of A^- after addition of NaOH = 2.5+0.75 = 3.25

Let's plug in the values again in Handerson equation:

pH=4.20+log(\frac{3.25}{4.25})

pH = 4.20 - 0.12

pH = 4.32

So, the pH of the buffer solution after addition of NaOH is 4.32.

7 0
3 years ago
QUESTION 1<br> Calculate the number of moles in 45.0 grams of C2H4O2.
yulyashka [42]

Answer:

0.749351061980325 moles (Exact)

0.75 moles (Rounded to the nearest hundredth)

Hope this Helps!

(Sorry if the answer is confusing)

5 0
2 years ago
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