What ratio of [A']/[HA] would be needed to prepare a buffer solution with a pH of 2.75 if the K, for HA is 4.0 * 10-4? O -0.65 O 3.4 O 0.22 O 4.4 -1.5
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![What ratio of [A]/[HA] would be needed to prepare a buffer
solution with a pH of 2.75 if the K, for HA is 4.0 * 104?
-0.65
3.4
0.22
O 4.4
O-1.5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2f591c64-216a-4120-ac44-1b23dfa641af%2F4d70abbb-dd73-4408-8e51-e092bfed1ce2%2F8c5qblo_processed.jpeg&w=3840&q=75)
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- A solution of is known to contain 0.100 M pyridine and 0.300 M pyridinum hydrochloride. The Kb for pyridine is 1.7 x 10-9 What is the pH of the solution?The Henderson-Hasselbalch equation gives a relationshipfor obtaining the pH of a buffer solution consisting of HA and A⁻. Derive an analogous relationship for obtaining the pOH of abuffer solution consisting of B and BH⁺.The value for is 6.38. What mole ratio of to is needed to prepare a buffer with a pH of 6.69?
- At what point will a buffer solution cease to moderate changes in pH? a. Only after all the acid or the base that needs to be buffered has been added. b. When waters equilibrium constant Kw has been reached. c. When the weak base acid and weak base salt concentration have been reached. d. When the acting buffering component is all neutralized.Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is 6x10-5) and 2.6g NaC6H5COOH in H2O. How much (in g) of the component of the buffer should be added in the 1000mL buffer so that its pH will be 3?10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
- Nitric acid (HNO3) and potassium hydroxide (KOH) both are considered as strong electrolytes. Discuss the titration curve (variation of pH with respect to addition of titrant) with suitable diagram and reactions involved when potassium hydroxide is added as titrant to HNO3 analyte.n a titration of 25.00 mL of X solution, 32.55 mL of 0.6896 M Y solution are required to reach the end-point. What is the concentration of the 25.00 mL of X?a. A formic acid/sodium formate buffer solution can be prepared with 0.012 M each offormic acid (HCOOH) and sodium formate (NaCOOH). The Ka for formic acid is1.8 x 10-4. The simultaneous equilibrium reaction is as shown below. Calculate the pH andthe buffer capacity of the solution.
- Identify the buffer capacity of the solution by titration using 0.250 M NaOH. Calculate the buffer capacity (β) of the phosphate buffer that have prepared using the data gathered below (see attached image): ΔpH = _____________________ ΔVNaOH = ___________________ Moles of titrant = ____________ Buffer Capacity (β) = _________What species are present in a solution giving off a pure blue endpoint in a hard water sample containing an EBT indicator (In) with an EDTA titrant? a. HIn²⁻, CaY²⁻, MgY²⁻ b. HIn²⁻, MgIn⁻, CaY²⁻, MgY²⁻, CaIn⁻ c. HIn²⁻, MgIn⁻ d. HIn²⁻, MgIn⁻, CaY²⁻If you were to overshoot tje endpoint in the titration of your unknown acid, would youncalculated molar mass be higher, lower or equal to the actual molar mass
