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A: There are several definitions for acids and bases, one of the definitions is that acid is species…
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A: 1. Concentration of hydrochloric acid = 0.015 M Hence [H3 O+ ] = 0.015M so, pH = -log[H3 O+ ] =…
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A: Equivalence point is point in titration at which the amount of titrant added is just enough to…
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A: A buffer solution is a solution which resist change in pH when small amount of an acid or base is…
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A: Number of moles =1721 millimoles ...Or because, 1milli = 10-3 so, = 1721 × 10-3 moles. = 1.721…
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Q: Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…
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Q: The pH of a solution that contains 1.2M acetic acid and 0.920M sodium acetate is?
A: pH of weak acid = 4.63.
Q: Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…
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A: The flow chart can be completed as: In 100 mL beakers, obtain 30 mL of the 0.1 M weak acid and 30 mL…
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A: The pH of the solution determines the concentration of H+ in the solution. A higher value of pH…
Q: Calculate the pH of a solution that is 0.135M benzoic acid and 0.260M sodium benzoate, a salt whose…
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Q: Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…
A: Given, 0.1 M solution of each species.
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A: HCOOH i.e, Formic acid would have been best choice pKa=1⋅77×10−4
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A: NaOH is a strong base , so we would first calculate its pOH using the formula : pOH = - log [OH-]…
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A: Given Concentration = 0.492 M pH = 10.46
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A: (1.) Given datas – [HCN] = 0.432 M pH = 4.868 -log [H+] = 4.868 [H+] = 10-4.868 [H+] = 1.355 ×…
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A: Let's first compare the substances, which are stronger acids than water.
Q: e pH at the equivalence point is
A: HCl is a strong acid and NaOH is a strong base
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Q: Consider the following data on some weak acids and weak bases:
A: Acid is the chemical species that increase the concentration of the positive ions in the solution…
Q: A 0.0001 molar basic solution is 1.50 % ionized. What is the pH of the solution if its Kb= ?
A: pH of solution is defined by the number of H+ present in the solution.
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A: As per the bartleby guidelines, am expert is allowed to answer one question at a time. Please re…
Q: The pH scale is only valid for water. Explain.
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- ans asap In the use of EDTA as the complexometric titrant, at what pH value/s does Y4- become a major component of solutions? -At pH 1 -At pH 7 -At pH values lower than 10 -At pH values greater than 104. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Calculate the ratio of the number of pink particles to the number of colourless particles of this indicator in a solution of pH = 9
- In the titration of 50.00mL of 0.2980M HCl, 71.93mL of 0.2173M NaOH was required to reach the phenolphthalien endpoint. Calculate the percent error between the predicted amount and the experimental amountA 250.0mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091M NAOH , requiring 29.5ml to reach end point. Determine equivalent weightTris(hydroxymethyl)aminomethane [(HOCH2)3CNH2—Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 × 10−6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer?
- 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.please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10concentration of I3- : 0.002M d. Titration data: Final volume: 29.05 mL Starting volume: 38.10 mL Delivered volume: 25.15 mL How do you calculate g?
- Imidazole (C3H4N2, MW = 68.07816, Kb = 9.80 x 10–8) can be used to create buffers at physiological pH’s. How many grams of imidazole and how many milliliters of 6.00 M HCl would be required to make 500.0 mL of 0.1000 M imidazole buffer with a pH of 7.20?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.