7. Given a buffer solution of sodium hydrogen carbonate (NaHCO3) and sodium carbonate (Na2CO3). a. Calculate...
7. Given a buffer solution of sodium hydrogen carbonate (NaHCO3)
and sodium carbonate
(Na2CO3).
a. Calculate the pH of this buffer solution when 0.100M sodium
hydrogen carbonate (NaHCO3)
and 0.100M sodium carbonate (Na2CO3). (Ka = 7.94 x 10-7)
b. Calculate the new pH value of this buffer solution when 1.00mL
of 0.100M NaOH is added to
to 100mL of this buffer
Homework Answers
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7. Given a buffer solution of sodium hydrogen carbonate (NaHCO3)
and sodium carbonate
(Na2CO3).
a. Calculate...
a) Buffer solutions with a pH values of around 10 are prepared using sodium carbonate (Na2CO3)...
a) Buffer solutions with a pH values of around 10 are prepared using sodium carbonate (Na2CO3) and sodium hydrogen carbonate (NaHCO3). What is the pH of a solution of 10.0g each of the two salts in enough water to make 0.250 L of solution? pKa2= 10.33 b) By how much does the pH change when 3.5mL of 6.0 M HCl is added? c) By how much does the pH of the solution change when 0.92 g of NaOH is added?
A buffer solution contains 0.386 M NaHCO3 and 0.233 M Na2CO3. Determine the pH change when...
A buffer solution contains 0.386 M NaHCO3 and 0.233 M Na2CO3. Determine the pH change when 0.055 mol HI is added to 1.00 L of the buffer. pH change = Determine the pH change when 0.117 mol NaOH is added to 1.00 L of a buffer solution that is 0.498 M in HCIO and 0.235 M in C10". pH after addition - pH before addition = pH change =
A buffer solution is prepared by dissolving 10.0 g of Na2CO3 and 10.0 g of NaHCO3...
A buffer solution is prepared by dissolving 10.0 g of Na2CO3 and 10.0 g of NaHCO3 in 0.250 L of water. What is the final pH of the solution you prepared? Ka = 4.67 x 10-11 Give a short explanation on how you would bring the pH of the above solution to 10 and confirm this
You are given sodium acetate, 1M HCl, NaHCO3, and Na2CO3. Determine which of these four would...
You are given sodium acetate, 1M HCl, NaHCO3, and Na2CO3. Determine which of these four would you need and then show calculations to make buffer pH=4.7 by the following: Strong Acid & Weak Base (mol/L)(g/mol)(L) = Weak Base Strong Acid: C1V1=C2V2 Assume making 100mL of a 0.1M buffer.
Solid sodium hydrogen carbonate, NaHCO3, decomposes on heating according to the equation: 2 NaHCO3(s) <-->...
Solid sodium hydrogen carbonate, NaHCO3, decomposes on heating according to the equation: 2 NaHCO3(s) <--> Na2CO3(s) + H2O(g) + CO2(g) A sample of 1.00 x 102 grams of solid NaHCO3 was placed in a previously evacuated rigid 5.00-liter container and heated to 160 0C. Some of the original solid remained and the total pressure in the container was 7.76 atmospheres when equilibrium was reached. Calculate the number of moles of H2O(g) present at equilibrium. How many grams of the...
A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate...
A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate to 1.00 L of 0.300 M sodium carbonate. What mass is required assuming the volume does not change? For carbonic acid, Ka1 = 4.45 x 10-7 and Ka2 = 5.69 x 10-11
Describe how to make 2.0L of a 2.00 M solution of sodium carbonate from solid sodium...
Describe how to make 2.0L of a 2.00 M solution of sodium carbonate from solid sodium carbonate(s). b. Describe how you can make a buffer with sodium carbonate(s) by adding hydrochloric acid. c. How many mL of 1.00 M HCl(aq) are needed to be added to 10.00 g of sodium carbonate to make a buffer at pH =10.00. Ka of HCO3- is 4.7 x 10-11.
A buffer solution contains 0.224 M NaHCO3 and 0.367 M Na2CO3. If 0.0485 moles of hydroiodic...
A buffer solution contains 0.224 M NaHCO3 and 0.367 M Na2CO3. If 0.0485 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH =
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.)
A buffer solution contains 0.69 mol of hydrogen peroxide (HOOH) and 0.39 mol of sodium hydrogen peroxide (NaOOH) in 6.60...
A buffer solution contains 0.69 mol of hydrogen peroxide (HOOH) and 0.39 mol of sodium hydrogen peroxide (NaOOH) in 6.60 L. The Ka of hydrogen peroxide (HOOH) is Ka = 2.4e-12. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.61 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.13 mol of HI?...
A buffer solution contains 0.386 M NaHCO3 and 0.233 M Na2CO3. Determine the pH change when 0.055 mol HI is added to 1.00 L of the buffer. pH change = Determine the pH change when 0.117 mol NaOH is added to 1.00 L of a buffer solution that is 0.498 M in HCIO and 0.235 M in C10". pH after addition - pH before addition = pH change =
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.)
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