Calculate the pH of a buffered solution that is prepared by dissolving 0.3 mol of NaHCO3 and 0.45 mol of Na2CO3 in 1 L of water at 298 K? (NaHCO3 pKa = 10.27)

Q: 1. Calculate the pH of an acetate buffer prepared by dissolving sodium acetate (5.21 g) and acetic…

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Q: The pH of a 0.50 M solution of an acid, HA, is 4.67. Calculate Ka of HA.

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Q: (Q24) What is the pH of a buffer solution that is 0.338 M in ammonia and 0.455 M in ammonium…

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Q: Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3-…

A: The given pKa1 is 6.1 Concentration of HCO3-is 0.024 M Concentration of H2CO3 is 0.0012 M a. pH of…

Q: A 0.20 M solution of niacin has a pH of 3.6. (a) What percentage of the acid is ionized in this…

A: Niacin is a weak acid. It is also known as nicotinic acid.Let us represent Niacin as HA, for better…

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

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Q: What is the pH of a solution that results from mixing together equal volumes of a 0.130 M  solution…

A: Given, 0.130 M solution of acetic acid 0.065 M solution of sodium hydroxide pKa of acetic acid =…

Q: Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M…

A: The relation between pH and concentration of  acid and its conjugate base is calculated using the…

Q: What is the pH of a solution that is 0.01M in picric acid and 0.1M in sodium picrate. (pKa=0.38)

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Q: If 90.00 mL of a 1.780 MHNO2 solution is reacted with 1.950g NaOH, calculate the resulting pH. The…

A: Given : Volume of HNO2 = 90 ml  Molarity of HNO2 = 1.780 M

Q: What is the pH of the solution containing 0.01 mol of CH3COOH and 0.820 grams of NaCH3COO in 100 mL…

A: Calculation of pH.

Q: How many grams of NaOH must be added to 1.50 L of a 0.400 M solution of oxoacetic acid (HCOCO2H) to…

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Q: NHa is a weak base (K = 1.8 × 10) and so the salt NH4CI acts as a weak acid. What is the pH of a…

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Q: A 0.15 M solution of an acid found in milk has a pH of 2.80. What is the percentage ionization of…

A: HA → H+ + A- The formula to calculate the pH is, pH= -log[H+] Therefore rearranging the formula let…

Q: The Ka of a monoprotic weak acid is 0.00244. What is the percent ionization of a 0.137 M solution of…

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Q: Don’t ever mix acid with cyanide (CN) because it liberates poisonous HCN(g). But, just for fun,…

A: (a)

Q: If 44.0mL of 0.20M HCI solution is titrated with 30.0mL of NaOH. what is the concentration of the…

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Q: What is the pKa of water if the ion product Kw is 1 × 10−14 and the concentration of pure water is…

A: We have to calculate the pKa of water.

Q: A solution containing 1.00 g NaCH3CH(OH)COO in 100.0 mL of 0.0500M CH3CH(OH)COOH has a pH of 4.11.…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH=pKa + log SaltAcid…

Q: Pyridine, C5H5N, is a pesticide and deer repellent, Its conjugate acid, the pyridinium ion C5H5NH+,…

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Q: At a certain point in a titration, 25 mL of 0.1M NaOH, has been added to 40 mL of a 0.1M solution of…

A: Buffer solution is defined as an aqueous solution which have weak acid and Conjugate of Strong base.…

Q: 9. An unknown salt is either: NaF, NaCl or NH,CI. When 0.1 mol of the salt is dissolved in 1.0 L of…

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Q: HASO HNO2 K = 5.0 x 10-3 K = 4.5x 104 1. You have a solution containing 70.0 mL of 0.40 M HASO and…

A: H3AsO4  is a weak acid. The solution of weak acid and its salt is called a buffer solution. The pH…

Q: HCN is a weak acid (?a=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: First write down the reaction between KCN and H2O. Then find OH- or H3O+ and using that find pH of…

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.120 M  solution…

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Q: Tris(hydroxymethyl)aminomethane [(HOCH₂)₃CNH₂,known as TRIS] is a weak base used in biochemical…

A: solution- auto dissociation of a compound is a temperature dependent process and the seperation…

Q: A 1.0 M solution of a weak acid, HA has a pH of 2.64. What is the value of Ka for this acid?

A: The acidic strength of all known acids is dependent on their dissociation constants. This constant…

Q: A 0.10 M solution of a weak acid HA has a pH of 2.80. What is the value of Ka for HA?

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Q: A 0.500M solution of a weak acid has a pH of 2.251. a. What is the pKa of the weak acid?

A: Given data Concentration of weak acid : C = 0.500 M pH of solution = 2.251  We know that for a weak…

Q: What is the pH of a buffer solution made by dissolving 0.11 mol of formic acid, HCOOH, and 0.12 mol…

A: Given: Moles of HCOOH = 0.11 moles Moles of HCOONa = 0.12 moles Volume of water = 1 L pKa of HCOOH =…

Q: What is the Ka or Kb expression for NH4Cl and Na2CO3? What is the value of Ka or Kb for both…

A: Salt hydrolysis: It is a reaction in which an acidic or basic solution is formed when one of the…

Q: If a 0.59 M solution of a monoprotic acid HA has a pH of 4.57, what is the Ka value of the acid HA?

A: Concentration of Acid HA = 0.59 M pH = 4.57     ICE Table:…

Q: . Novocain, the commonly used local anesthetic, is a weakbase with Kb = 7 × 10-6 M. (a) If you had a…

A: (a) Given for the weak base: concentration = 0.0200M Kb = 7 × 10-6 We know that, for the weak base,…

Q: Carbonic acid (H2CO3) and bicarbonate ion (HC0;) are used as a buffer system to regulate the blood…

A: Given,  Ka of H2CO3 = 4.2 x 10-7  pH = 7.15

Q: Calculate the pH of a buffer solution made by dissolving 50 g of NaHCO3 and 20 g of H2CO3 to make…

A: Answer :-  (b) 6.63  the pH of a buffer solution made by dissolving 50 g of NaHCO3 and 20 g of H2CO3…

Q: 2. A 0.100 mole quantity of a monoprotic acid HA is added to 1.00 L of pure water. When equilibrium…

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Q: Calculate the pH of a buffer solution made by dissolving 50.0 g of NaHCO3 and 20.0 g H2CO3 to make…

A: 1- First we will determine the moles of acid and salt :  a) moles of acid = [ mass / molar mass of…

Q: What is the pH of a solution when 82.5 mL of a 0.1M HCN solution (ka = 6.2 x 10 -10) is titrated…

A: pH of a solution is the negative logarithm of the H+ ion concentration. In acid-base titrations, one…

Q: A buffer solution is prepared by dissolving  1.700 g of ammonium chloride (NH4Cl) into 100.00 mL of…

A: Mass of ammonium chloride is 1.7 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: Determine the pH of a solution made by adding 0.30 mol of acetic acid (CH3COOH) and 0.30 mol of…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: 3) What is the pH of a 0.1OM solution of NaCN? The K, of HCN is 4.9 x 10-10. la. 2.85 b. 5.15 C.…

A: The salts that are formed from the strong acids and strong bases would not undergo hydrolysis. The…

Q: The pH of a 0.800 M aqueous solution of a weak acid is 1.99. What is the value of Ka for this acid?

A: Given  pH = 1.99 Concentration (c) = 0.800 M Ka =?

Q: Assuming that an acid (AH) which has pKa=6.4 is added to the buffered solution with pH=5.8.…

A: pKa of HA = 6.4 Calculation of Ka: pKa=-log Ka6.4=-log KaKa=10-6.4=3.981×10-7 Calculation of [H+]:…

Q: A phosphate buffer is prepared by mixing 200. mL of 0.250 M KH2PO4 and 300. mL of 0.400 M K2HPO4.…

A: Given : Molarity of Acid = 0.250 M Molarity of Base = 0.400 M Volume of Acid = 200 mL Volume of Base…

Q: 1. Calculate the pH of a solution prepared by mixing 300 Ml of 0.10 M HF and 200 Ml of 0.10 M KOH.…

A: In chemistry , If pH of the solution has to be determined ,     Henderson- Hasselbalch equation will…

Q: If 50.00 mL of a 0.1000 M hydrochloric solution is titrated with a 0.0985 M NaOH solution, what is…

A: Volume of hydrochloric solution=50.0mL Concentration of hydrochloric solution=0.1000M Concentration…

Q: Hypobromous acid, HBrO, can be produced commercially as a disinfectant. A solution is made by…

A: HBrO is a weak acid.  pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: Calculate the ratio of conjugate base to weak acid, [A−]/[HA], needed to make a buffer at pH = 5.00…

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Q: What is Ka for a weak monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28 at 25°C?

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.