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A: As 0.36M of sodium formate of 20.0 ml is mixed with 0.18 M of HCl of 40.0 mL, thus equivalence point…
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A: Since you have posted multiple questions which are not sub-parts, we are entitled to answer the…
Q: 0.100
A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid
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A: Blank solution means it has absence of analyte substance.
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A: H3PO4 decomposes as follows:
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Q: Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a…
A: Mixing of 68ml 0.17M ammonia and 42 ml 0.13 M ammonium chloride.
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A: Equilibrium is a condition at which rate of forward as well as backward reaction is same. Common ion…
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A: pH of 0.100 M HCl = 1.092 pH = - log aH+ Activity of H+ = 10-1.092…
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Q: A 25.00 ml solution of 0.1000 M HF, hydrofluoric acid (Ka 6.8 x 104) is added to 12.50 mL solution…
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Q: A chemist titrates 130.0 mL of a 0.8883 M ammonia (NH2) solution with 0.0816 M HC1 solution at 25…
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A: Reaction: H2Ox + OH- —->HOx- + H2OHOx- + OH- ——->Ox- + H2O Equilibrium: H2Ox ——>HOx- + H…
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Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10~7. Calculate the pH of a 4.0…
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Q: Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak base (molar mass =…
A: Given :- Mass of weak base = 0.0925 g Molar mass of weak base = 17.03 g/mol Volume of water = 100 mL…
Q: Calculate the % relative error in hydronium ion concentration by using concentrations instead of…
A: Given Ka, Acetic Acid → 1.75×10-5 Ammonium ions → 5.70×10-10 Chloroacetic Acid → 1.36×10-3…
Q: It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3COO should be…
A: Given;
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Q: Calculate the pH of a 0.10 M NaCN solution. Ka of HCN = 6.2 x 10-10
A: Given: Concentration of NaCN = 0.1 M Ka of HCN = 6.2 x 10-10 To calculate: pH =?
Q: For a solution that is 0.50 M in NH3 (Kb =1.8 x 10-5) and 0.25 M in NH4Cl, find pH and pOH
A: The Henderson-Hasselbalch equation is given as,
Q: Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2…
A: Given, Concentration of H2A, [H2A] = 0.10M a. Ka1 = 1.0 X 10-4; Ka2 = 5.0 X 10-5b. Ka2 = 1.0 X 10-4;…
Q: Magnesium carbonate is slightly soluble in water. The Ksp for MgCO3 is 3.5 x 10-8. The carbonate ion…
A: Given, For, MgCO3 Ksp=3.5×10-8 pH=7.5
Q: Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary…
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Q: Calculate the pH and [H3O+] of a solutio n prepared by dissolving 0.25 mol of NaC2H3O2 in 500. mL of…
A: For a buffer solution: pH = pKa + log[salt]/[acid]
Q: The pH of 0.200moldm-3 solution of the weak base pyridine, C5H5N is 8.59.Draw up a concentration…
A: We have to calculate the Kb.
Q: What is the concentration of hydroxide ions in pure water at 30.0∘C, if Kw at this temperature is…
A: The ionization of water is represented as,
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- Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3 with deonised water.A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.Calculate the pH of a 2.2 M solution of pyridine salt (Kb (pyridine) = 1.7 x 10-9). Using the structure of pyridine (in image attachment) react pyridine with acetic (ethanoic) acid in a Bronstead-Lowry reaction. Use curved arrows to show the exchange of the proton, and label the conjugate acid base pairs.
- Write equilibrium showing the carbonate anion (CO32-) acting as a Brønsted base in aqueous solution. Identify the conjugate base-acid (or acid-base) pairs and write the appropriate base dissociation constant (Kb) expression. Look up Kb value and compare to Kb of carbonate as 2.1 x 10-4. Did your value fall in the same range?Rainwater is acidic because CO2(g) dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Calculate the concentrations of carbonic acid, bicarbonate ion (HCO3-) and carbonate ion (CO32-) that are in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 * 10-5 M.Using the Henderson-Hasselbach equation, determine the pKa of a fictitious equilibrium solution with the weak acid (HA) having a concentration of 0.08M, the base (A-) having a concentration of 0.02M at a pH of 1.9.
- The acid-dissociation constants of phosphoric acid (H3PO4) at 25 degrees Celsius are Ka1 = 7.510-3, Ka2 =6.2 10-8, and Ka3 =4.210-13. What is the PH of a 2.5M aqueous solution of phosphoric acid?A particular solution is 0.05M with respect to ethanoic acid and 0.2M with respect to sodium ethanoate (Ka for ethanoic acid = 2 x 10-5moldm-3). What is this type of solution called? Calculate the pH of the solutionThe acid dissociation constant for acetic acid (HC2H3O2, commonly abbreviated HAc) is 1.8 x 10-5. Calculate the pH of a 0.10 M solution of HAc.
- Write the chemical equation and the Ka expression for theacid dissociation of each of the following acids in aqueoussolution. First show the reaction with H+(aq) as a productand then with the hydronium ion: (a) C6H5COOH,(b) HCO3-.Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.425 M HCl. With 0.0162 moles of H⁺ in excess in a volume of 175.0 mL, what would be the pH of this solution after the reaction?In theory the pH of distilled water will be 7 or slightly less…why?
