Question
In: Chemistry
A 100.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. A....
A 100.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br.
A. What mass of HCl could this buffer neutralize before the pH fell below 9.00
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?
I know for A i have tried .19g, .0915, and .5`3 using three different methods. I have no idea what to do now.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. A)...
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in
NH4Br. 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 0.250 M
in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled
before the pH falls below 9.00?
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. A)...
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in
NH4Br.
A) What mass of HCl could this buffer neutralize before the
pH fell below 9.00? answer to this was
0.088g
B) If the same volume of the buffer were 0.265 M in NH3 and
0.395 M in NH4Br, what mass of HCl could be handled before the pH
fell below 9.00?
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br. What...
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in
NH4Br. What mass of HCl can this buffer neutralize before the pH
falls below 9.00? If the same volume of the buffer were 0.250 M in
NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before
the pH falls below 9.00? Need answer in grams. PS the answer is not
.092
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.135 M in NH4Br. A)...
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.135 M in
NH4Br.
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 0.270 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 0.105 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 0.100 M in NH3 and 0.135 M in NH4Br. a.Part...
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.135 M in
NH4Br. a.Part A What mass of HCl can this buffer neutralize before
the pH falls below 9.00? b.Part 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?
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 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=?
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