Given: for terephthalic acid, H2CSH.O4 Kai = 3.1 x 10 4; Ka2 =1.5 x 10 5 Solve for the expected numerical pH values two places beyond the decimal for the first and second half equivalence points and use that to determine the pH at the first equivalence point for the salt NaH:CsH.O4, First equivalence point pH value?
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Q: Write your answer in the space provided. Show your calculations to get full credit. A 1.0 M…
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Q: is reached: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 50.0 mL…
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Q: (a) Please write the conjugate bases of the following acids. (1) CH3COOH - CH3CO0 (Ka = 1.76 x 10-5)…
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Q: What is the pH of a 0.710 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?
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Q: The pH for 0.0850 M solution of C6H:CH2COOH is 2.68. Determine the value of Ka for CsHsCH2COOH. PREV…
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Q: CH3CH₂COOH(aq) + H₂O(l) → CH3CH₂COO (aq) + H30* (aq) Propanoic acid, CH3CH₂COOH, is a carboxylic…
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Q: pH calculation before the first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic…
A: Solved in step 2.
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Q: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M…
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- The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.a. Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. b. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surely
- MUST ANSWER BOYH SUBPARTS A AND B A 1.161g sample of pure maleic acid (H2M, 116.1 g/mol) with Ka1 and Ka2 values of 1.42 × 10-2 and 8.57 ×10-7, respectively, was contained in a 100.0 mL solution with a pH of 5.0. In solution, maleic acid can dissociate into HM- and M2- species. The three species (H2M, HM- and M2-) exist in the solution at varying concentrations that depend on the pH of the solution. a) Calculate the values of α1 (alpha 1) and α3 (alpha 3). b) Calculate the concentration of HM- in the above solution.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.find Ka for acetic acid from following half equivalence data point of half equivalence : 5 mLhalf equivalence pH value: 0.88concentration of NaOH: 0.99/ mol L-1 Volume of NaOH at equivalence point: 10mLVolume of acetic acid/mL: 40 mL
- A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?How to answer for Ka/ Kb and calculated pH of a solution?I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Given: In a 10.0 mL 0.10 M CH3COOH solution, a 15 mL 1.00 M HCl solution was added. Compute for it's ka/kb and pH.
- v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH at 25oC is 1.76 x 10-5.Hydrogen sulfide (H2S) is an odorous gas that can be stripped from solution by bubbling air through the solution. H2S when dissolved in water is also a weak acid that can deprotonate to bisulfide ions which are not removed by air stripping. That reaction is ?2?--> H^+ + ??^- With equilibrium constant Ka=0.86x10-7.Find the fraction of hydrogen sulfide in the H2S form at pH 6 and pH 8. At which pH would you expect to have an easier time to strip away H2S gas?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. HCOOH (aq) + H2O (l) ⇋ H3O+ (aq) + HCOO- (aq)