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 =

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.

Ascorbic acid (vitamin C, H2C6H6O6)  is widely used in many food products. A solution of  0.1 M of ascorbic acid Ka1 = 7.9x10-5 and Ka2 = 1.6x10-12 is made, what is the concentration (in M) of ascorbate ion C6H6O62- H2C6H6O6(aq) + H2O(I) <---> H3O+(aq) + HC6H6O6-(aq) HC6H6O6-(aq)+ H2O(I) <---> H3O+(aq) + C6H6O62-(aq)     Question options:   1.6X10-12   5.9X10-12   3.7X10-12   2.3X10-12   6.3X10-12

(3) 11. In a titration it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution. Show your work. [Hint: Write a balanced equation for the reaction first.]

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.

if 25.0g of NaOH is added to 0.750L of 1.00M Cd(NO3)2 how many grams of Cd(OH)2 will be fromed in the following precipitation reaction? 2 NaOH9aq)+ Cd(NO3)(aq)= Cd(OH)2(s)+ 2NaNO3(aq)

please answer only d and e in question