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algol [13]
3 years ago
14

What is the ph of a 0.15 m solution of ammonium chloride?

Chemistry
1 answer:
Thepotemich [5.8K]3 years ago
7 0
 Best Answer:  <span>(a) 
8.9 x 10^-7 = x^2 / 0.15-x 
x = [OH-] = 0.00037 M 
pOH = 3.4 
pH = 14 - 3.4 = 10.6 

(b) 
Ka = Kw/Kb = 5.6 x 10^-10 = x^2 / 0.20-x 
x = [H+] = 0.000011 M 
pH = 5.0</span>
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Q6. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 86.4 mL of 0.494 M H2SO4. Calculate the
skelet666 [1.2K]

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The correct answer should be 12.72 pH of the mixed solution and 9.94g mass of solid BASO4 formed.

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0.0426816<--- 0.0426816

The mixed solution is Ba(OH)2 with 0.05 - 0.0426816 = 0.0073184

The concentration of mixed solution is : 0.0073184 : ( 0.05 + 0.0864 ) = 0.054 M

The pH of mixed solution is 14 - -log[0.054] = 14 - 1.27 = 12.73 PH

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6 0
3 years ago
If I have an unknown quantity of gas at STP with a volume of 41 liters, how many moles of gas do
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8 0
3 years ago
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