Here is the updated version (1). A buffer solution is made that is 0.458 M in...
Here is the updated version
(1). A buffer solution is made that is 0.458 M in H2CO3 and 0.458 M in KHCO3 .
If Ka1 for H2CO3 is 4.20 x 10^-7, what is the pH of the buffer solution? pH = _____
Write the net ionic equation for the reaction that occurs when 0.104 mol HCl is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+)
____ + ____ --> ____ + ____
(2). Write a balanced net ionic equation to show why the
solubility of
Pb3(PO4)2(s) Ksp=
3.0 x 10^-44 increases in the presence of a strong acid and
calculate the equilibrium constant for the reaction of this
sparingly soluble salt with acid.
Consider only the FIRST STEP in the reaction with strong acid. Use
the pull-down boxes to specify states such as (aq) or (s).
| _____(aq)(s)(l)(g) |
+ |
_____(aq)(s)(l)(g) | ----> | _____(aq)(s)(l)(g) |
+ |
____(aq)(s)(l)(g) |
+ |
____(aq)(s)(l)(g) |
K = ____
Homework Answers
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Here is the updated version
(1). A buffer solution is made that is 0.458 M
in...
Part A) A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M...
Part A) A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M in NaHCO3. If Ka1 for H2CO3 is 4.20 x 10^-7 , what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) PART B) A buffer solution is made that is 0.311 M...
A buffer solution is made that is 0.366 M in and 0.366 M in . If...
A buffer solution is made that is 0.366 M in and 0.366 M in . If Ka1 for H2CO3 is 4.20*10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.098 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
Use the References to access important values if needed for this question. A buffer solution is...
Use the References to access important values if needed for this question. A buffer solution is made that is 0.458 M in H, CO3 and 0.458 M in NaHCO3 If Kal for H2CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.135 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use...
A buffer solution is made that is 0.491 M in H2S and 0.491 M in KHS...
A buffer solution is made that is 0.491 M in H2S and 0.491 M in KHS If Ka1 for H2S is 1.00 x 10, what is the pH of the buffer solution? pH= Write the net ionic equation for the reaction that occurs when 0.102 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS....
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS. If Kal for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.129 mol HI is added to 1.00 L of the buffer solution instead of H (Use the lowest possible coefficients. Omit states of matter. Use H30 Submit Answer Retry Entire Group 9 more group attempts remaining...
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3...
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3 . If Kal for H,CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH=) Write the net ionic equation for the reaction that occurs when 0.133 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
Use the References to access important values if needed for this question. A buffer solution is...
Use the References to access important values if needed for this question. A buffer solution is made that is 0.339 M in H, CO3 and 0.339 M in NaHCO3 If K1 for H2CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.082 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H0+...
this is part a,b,c of one question. please answer all parts or leave to another tutor....
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
A buffer solution is made that is 0.368 M in HCIO and 0.368 M in NaClO....
A buffer solution is made that is 0.368 M in HCIO and 0.368 M in NaClO. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.089 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) -
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS....
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
Use the References to access important values if needed for this question. A buffer solution is made that is 0.458 M in H, CO3 and 0.458 M in NaHCO3 If Kal for H2CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.135 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use...
A buffer solution is made that is 0.491 M in H2S and 0.491 M in KHS If Ka1 for H2S is 1.00 x 10, what is the pH of the buffer solution? pH= Write the net ionic equation for the reaction that occurs when 0.102 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS. If Kal for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.129 mol HI is added to 1.00 L of the buffer solution instead of H (Use the lowest possible coefficients. Omit states of matter. Use H30 Submit Answer Retry Entire Group 9 more group attempts remaining...
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3 . If Kal for H,CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH=) Write the net ionic equation for the reaction that occurs when 0.133 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
Use the References to access important values if needed for this question. A buffer solution is made that is 0.339 M in H, CO3 and 0.339 M in NaHCO3 If K1 for H2CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.082 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H0+...
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
A buffer solution is made that is 0.368 M in HCIO and 0.368 M in NaClO. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.089 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) -
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
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