Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO₂. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? OH(aq) + HCHO, (aq) → CHO2 (aq) + H2O() NaOH(aq) + HCHO₂ (aq) NaCHO₂ (aq) + H₂O(1) OH(aq) + H3O+ (aq) → 2H₂O(1) NaOH(aq) + H3O+ (aq) → Na (aq) + 2H₂O(1)

+ Titration of Weak Acid with Strong Base A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA (aq) + OH (aq) →A (aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 106, is titrated with NaOH. Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit Part B pH = VE ΑΣΦ More strong base added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 42.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IV— ΑΣΦ Submit ? 16 of 3 Review | Constants | Periodic

Write a balanced molecular equation for the reaction that occurs when aqueous solutions of sodium hydroxide, NaOH, and hydrochloric acid, HCl, are combined. It is not necessary to include states such as (aq) or (g). + +

The pH of an aqueous solution of 8.39×10-2 M ammonium nitrate, NH4NO3 (aq), is

Calculate the concentration of HS in an aqueous solution of 0.142 M hydrosulfuric acid, H₂S (aq). [HS] = M.

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.

B). Is solution, acidic, neutral or basic?

Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pK, = 4.75) with 0.131 M NaOH. CH;COOH(aq)+NaOH(aq) · CH, COO (aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH : Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =

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.

a Ammonium chloride and rubidium acetate, RbCH, CO₂, are mixed in water. Choose a balanced equation for the acid-base reaction that could, in principle, occur. O RbCH3CO₂ (s)+NH, Cl(s) + H₂O() = Rb+ (aq) + CH3CO₂¯(aq) +NH, +(aq) +Cl¯(aq) OCH3CO₂ (aq) + NH4+ (aq) CH3CO₂H(aq) + NH3 (aq) RbCH, CO₂ (aq) + NH4Cl(aq) NH₂CH3 CO₂ (aq) + RbCl(aq)