Citric acid/citrate buffer is a pH buffer that is used for baby locations. A pH buffer is prepared by dissolving 17.77 grams C6H5O7Na2 and19.67 grams of C6H4O7Na3 in enough water to make 250.0 mL solution.C6H40 (aq) + H30¹ (1)C6H₂O² (aq) + H₂O(1)The 3rd acid dissociation constant of citric acid is 4.012×10-7.Please answer the following questions.A.B.What is the pH of the solution? pH =Please provider your answer below.0²If you add 5.000 mL, 0.5363 M of HC1 to 250.0 mL above solution you prepared, what will be the final pH? Assume that thevolume is additive. pH =Please provider your answer below.00→→ $ □C.If you add 5.000 mL, 0.5363 M of Ba(OH)₂ to 250.0 mL above solution you prepared, what will be the final pH? Assume thatthe volume is additive. pH =Please provider your answer below.→→ $$

we have to calculate the pH of solution

Citric acid/citrate buffer is a pH buffer that is used for baby locations. A pH buffer is prepared by dissolving 17.77 grams C₂H5O7Na₂ and 19.67 grams of C6H₂O7Na3 in enough water to make 250.0 mL solution. C6H₂O3(aq) + (aq) + H₂O(1) C6H₂O(aq) + H₂0 (1) The 3rd acid dissociation constant of citric acid is 4.012×10-7. Please answer the following questions. A. What is the pH of the solution? pH =

Citric acid/citrate buffer is a pH buffer that is used for baby locations. A pH buffer is prepared by dissolving 17.77 grams C₂H5O7Na₂ and 19.67 grams of C6H₂O7Na3 in enough water to make 250.0 mL solution. C6H₂O3(aq) + (aq) + H₂O(1) C6H₂O(aq) + H₂0 (1) The 3rd acid dissociation constant of citric acid is 4.012×10-7. Please answer the following questions. A. What is the pH of the solution? pH =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50.mL of a 0.081 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
Sodium hydrogen carbonate (NAHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: 圖 HCl(aq) + NaHCO,(aq) → NaCl(aq) + H,O(1) + CO,(g) ol. The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 250. mL of a 0.065 M HCl solution. What mass of NaHCO, would she need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
The following two solutions are mixed together: 125.0 mL of 0.2798 MPb(C2H3O2)2(aq) and 275.0 of 0.1901 M KCl(aq)Pb(C2H3O2)2(aq) + 2 KCl(aq) → PbCl2(s) + 2 KC2H3O2(aq)Determine the final concentration of K+ and Pb2+ in solution. Assume the volumes areadditive.
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A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10–4 Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer.
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150.mL of a 0.045 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
Codeine, C18H26O3N is the active ingredient in the sedative Paregoric™ and is a weak Brønsted base with Kb = 8.9 x 10–7 (conjugate acid is C18H26O3NH+). To a 20.00 mL sample of 0.0155 M aqueous solution of Codeine is added 9.75 mL of 0.0180 M HCl(aq). a) Calculate the pH of the above solution. b) To the above solution is added 1.00 mL of 0.0150 M NaOH(aq). Calculate the new pH that results and the % change in pH. Show your work and justify any approximations made.
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO2(g) ->> The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.089 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCI? Round your answer to 2 significant digits. x10 x
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)⟶CO2(g)+H2O(l)+CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 15.0 mL of a solution that is 0.500 M in HCl, how many grams of CO2 gas are produced? Express the mass to three significant figures and include the appropriate units.
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