A volume of 500.0 mL of 0.110 M NaOH is added to 525 mL of 0.250 M weak acid (Ka = 2.53 × 10-'). What is the pH of the resulting buffer? НА(аq) + ОН (aq) Н,О() + А (аq) >
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- A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
- A buffer solution contains 0.31 mol of phenol (HC6H5O) and 0.85 mol of sodium phenoxide (NaC6H5O) in 4.00 L.The Ka of phenol (HC6H5O) is Ka = 1.3e-10.(a) What is the pH of this buffer?pH = _______ (b) What is the pH of the buffer after the addition of 0.27 mol of NaOH? (assume no volume change)pH = ______(c) What is the pH of the original buffer after the addition of 0.62 mol of HI? (assume no volume change)pH = _______NaOH (ag) + HKCgHO4 (ag) -- NakCgHO4 laa) • HyO () 1.557 gof KHP is dissolved in 25.00 ml of water with 2 drops of indicator. NaOH is added to a burette. Shown below are pictures of the burette before the titration has begun (initial reading) and after the endpoint of the titration has been reached (hnal reading). Burette before titration (Initial reading, mL) Burette aftertitration (Final reading mL) 28 46 29 30 On your scratch paper, answer the following questions: A. Record the volume of NaOH to the correct number of sig figs in the burette before the titration. B.Record the volume of NaOH to the correct number of sig figs in the burette after the titration. C. What is the volume of NaOH required to reach the endpoint of the titration? Use correct significant higures D. Calculate the original molarity of the NaOH Enter your final answer in the blank below to the correct number of significant fgures Show your workA buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen sulfide (NaHS) in 8.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?pH = ____(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)pH = ____(c) What is the pH of the original buffer after the addition of 0.02 mol of HI? (assume no volume change)pH = ____
- A volume of 500.0 mL of 0.130 M NaOH is added to 605 mL of 0.200 M weak acid (Ka = 3.87 × 10-5). What is the pH of the resulting buffer? HA(aq) + OH(aq) · H,O(l) + A-(aq) pH = TOOLS V1 attempts left Check my work Enter your answer in the provided box. A buffer solution is prepared in such a way that the concentration of propanoic acid is 1.8 x 10 M and the concentration of sodium propanoate is 1.9 x 10° M. The buffer equilibrium is described by Guic C,H;COOH(aq) + H2O(1) =H,o*(aq) + C,H3CO0aq) propanoic acid propanoate ion with K 1.34 x 10P. If the concentration of the sodium propanoate were doubled while the acid concentration remained the same, calculate the pH of the resulting solution. pH =ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-
- (a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after the addition of 0.030 mol HCl? note: Ka (NH4+) = 5.6 x 10 -10 NH3 (aq) + H+ (aq) → NH4+ (aq) (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.1. Consider the titration of 25.0 mL of a weak acid, 0.100 M HCOOH (Ka = 1.8 x 10- 4) with 0.100 M NaOH. NaOH (aq) + HCOOH(aq) →H2O(1) + NaCHO2(aq) (i) What is the pH of the solution after adding 5.00 mL of NAOH? (ii) After adding 12.5 mL 2 Veq= midpoint pH = pKa = 3.74You have75.0 mL of a 0.25M solution of a weak base, ethanol amine, HOC2H4NH2, with a kb= 2.8x10^-5. It is to be titrated with 0.50 M HCl. What is the pH of the resulting solutions after the following additions? (a) initial pH (B)after 10.50 mL of HCl have been added (c) 1/2 way to the equivalence point (d) at the equivalence point (E) after 40 mL of HCl has been added (f) what indicator would you choose to signal the endpoint, and WHY?