Question
In: Chemistry
A 110.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125 molL−1 in NH4Br. Part...
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A 110.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125 molL−1 in NH4Br. |
Part A (PLEASE ANSWER EVERY PART CORRECTLY :)) What mass of HCl will this buffer neutralize before the pH falls below 9.00? (Kb(NH3)=1.76×10−5 Express your answer using two significant figures.
Part B If the same volume of the buffer were 0.265 molL−1 in NH3 and 0.390 molL−1 in NH4Br, what mass of HCl could be handled before the pH fell below 9.00? Express your answer using two significant figures.
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Solutions
Expert Solution
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queen_honey_blossom answered 2 years agoRelated Solutions
A 110.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125 molL−1 in NH4Br. (A)...
A 110.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125
molL−1 in NH4Br.
(A) What mass of HCl will this buffer neutralize before the pH
falls below 9.00? (Kb(NH3)=1.8×10−5)?
(B) If the same volume of the buffer were 0.265 molL−1 in NH3
and 0.390 molL−1 in NH4Br, what mass of HCl could be handled before
the pH fell below 9.00?
#6. A 130.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125 molL−1 in NH4Br....
#6. A 130.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.125
molL−1 in NH4Br.
A) What mass of HCl will this buffer neutralize before the pH
falls below 9.00? (Kb(NH3)=1.76×10−5)
B)If the same volume of the buffer were 0.270 molL−1 in NH3 and
0.390 molL−1 in NH4Br, what mass of HCl could be handled before the
pH fell below 9.00?
A 110.0 −mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. Part...
A 110.0 −mL buffer solution is 0.110 M in NH3 and 0.135 M in
NH4Br.
Part A What mass of HCl could this buffer neutralize before the
pH fell below 9.00? Express your answer using two significant
figures.
m=?
Part B If the same volume of the buffer were 0.265 M in NH3 and
0.390 M in NH4Br, what mass of HCl could be handled before the pH
fell below 9.00? Express your answer using two significant
figures.
m=?
A 120.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.135 molL−1 in NH4Br. If...
A 120.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.135
molL−1 in NH4Br. If the same volume of the buffer were 0.255 molL−1
in NH3 and 0.400 molL−1 in NH4Br, what mass of HCl could be handled
before the pH fell below 9.00?
the answer is not 0.084g!
A 100.0 −mL buffer solution is 0.110 M in NH3 and 0.125 M in NH4Br. A....
A 100.0 −mL buffer solution is 0.110 M in NH3 and 0.125 M in
NH4Br.
A. If the same volume of the
buffer were 0.260 M in NH3 and 0.395 M in NH4Br, what mass of HCl
could be handled before the pH fell below 9.00?
B. What mass of HCl could this buffer neutralize before the
pH fell below 9.00?
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.135 molL−1 in NH4Br. What...
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.135
molL−1 in NH4Br. What mass of HCl will this buffer neutralize
before the pH falls below 9.00? (Kb(NH3)=1.8×10−5). If the same
volume of the buffer were 0.270 molL−1 in NH3 and 0.400 molL−1 in
NH4Br, what mass of HCl could be handled before the pH fell below
9.00.
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in
NH4Br. (Kb of NH3 is 1.76×10−5.)
a.)What mass of HCl can this buffer neutralize before the pH
falls below 9.00?
b.)If the same volume of the buffer were 0.255 M in NH3 and
0.400 M in NH4Br, what mass of HCl could be handled before the pH
falls below 9.00?
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M
in NH4Br. (Kb of NH3 is 1.76×10−5.)
a.)What mass of HCl can this buffer neutralize before the pH
falls below 9.00?
I already did this and got 0.101 g, which is right, but I am
struggling to answer Part B.
b.)If the same volume of the buffer were 0.255 M in NH3
and 0.400 M in NH4Br, what mass of HCl could be handled before the
pH...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in
NH4Br. (Kb of NH3 is 1.76×10−5.)
If the same volume of the buffer were 0.255 M in NH3 and
0.400 M in NH4Br, what mass of HCl could be handled before the pH
falls below 9.00?
Please help me figure out the answer! I am on my last attempt. I
have entered the following answers and these are NOT correct:
0.0916, 0.0915, 0.094, 0.101, 0.999, 0.0999,...
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. What...
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.125 M in
NH4Br. What mass of HCl can this buffer neutralize before pH falls
below 9.00? Please help and show work. I keep getting 2.5-2.85 g of
HCl. I cannot figure this out, it keeps saying its the incorrect
answer!
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