Phosphoric acid is a triprotic acid (Ka1=6.9×10−3Ka1=6.9×10−3, Ka2=6.2×10−8Ka2=6.2×10−8, and Ka3=4.8×10−13Ka3=4.8×10−13). To find the pH of a buffer composed of H2PO−4(aq)H2PO4−(aq) and HPO2−4(aq)HPO42−(aq), which pKaKa value should be used in theHenderson–Hasselbalch equation? pKa1Ka1 = 2.16 pKa2Ka2 = 7.21 pKa3Ka3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 27.027.0 g of KH2PO4(s)KH2PO4(s) and 45.045.0 g of Na2HPO4(s)Na2HPO4(s) in water and then diluting to 1.00 L.

Q: 18.63 mL of 0.100M H2SO4(aq) is placed in a beaker.  After 16.42 mL of NaOH is added to the beaker,…

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Q: What is the pH of a buffered system made by dissolving 17.42 g of KH2PO4 (MM 136.1 g/mol) and 20.41…

A: Given : Mass of KH2PO4 = 17.42 g Mass of K2HPO4 = 20.41 g And Ka of KH2PO4 = 6.2 X 10-8  Molar mass…

Q: Which of the following solutions could be a buffer?     hydrochloric acid/hydrobromic acid;…

A: Buffers can be classified into three types according to their constituents: (1) Weak acid and a salt…

Q: A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36)…

A: PH+Poh=14. This is basic buffer equation  Poh=pkb+log[salt]/base Use this equation and get the…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has:Concentration of NH4Cl/NH4+ = 0.181 MConcentration of NH3 =…

Q: A chemistry graduate student is given 100.mL of a 0.40M trimethylamine ((CH3)3N) solution.…

A: Given : concentration of (CH3)3N = 0.40 M volume of (CH3)3N solution = 100 mL = 0.1 L…

Q: Consider a buffer solution containing 0.040 M ammonia (NH3) and 0.060 M ammonium chloride (NH4Cl).…

A: Ka = 5.70*10-10 Volume of NaOH = 5 mL Molarity of NaOH = 1M Concentration of NH3 = 0.040M…

Q: Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and…

A: The Ka values for the phosphoric acid areThe phosphoric acid has the following ionizations  H3PO4 ⇌…

Q: A buffer is made by adding 0.68 g of sodium formate, NaHCOO (molar mass = 68.0 g/mol), to 1.00 L of…

A: Given : Mass of sodium formate i.e NaHCOO = 0.68 g Concentration of formic acid i.e HCOOH = 0.015 M…

Q: Calculate the change in pH when 9.00 of 0.100 M HCl * (aq) is added to 100.0 of a buffer solution…

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Q: Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution…

A: Given that,    Volume of 0.100 M HCl = 7.0 mL  = 0.007 L   Moles of HCl in 7 ml = 0.100 M×0.007 L =…

Q: The conjugate base, A⁻ of a certain weak acid, HA has the molar mass 67.997 g/mol. What mass of this…

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Q: A buffer solution is prepared by adding 12.71 g of sodium acetate (NaC2H3O2) and 15.98 g of acetic…

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Q: A chemistry graduate student is given 100. mL of a 0.90M trimethylamine ((CH3)₂N) S solution.…

A: Volume of trimethylamine, solution = 100 mLConcentration of trimethylamine solution = 0.90 MThe…

Q: One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0…

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Q: A buffer solution is prepared by adding 14.98 g of sodium acetate (NaC2H3O2) and 15.33 g of acetic…

A: Given, mass of sodium acetate = 14.98 g mass of acetic acid = 15.33 g volume = 500 mL = 0.5 L Ka…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: A buffer solution is prepared in such a way that the concentration of propanoic acid is    8.0 ×…

A: Given, Ka = 1.34 ×10−5   C2H5COOH(aq)  +  H2O(l)  ⇌  H3O+(aq)  +  C2H5COO−(aq) propanoic acid…

Q: Calculate the pH of a solution of magnesium hydroxide, Mg(OH)2 (Ksp = 5.6 × 10−12), made by…

A: Solubility Product : For a sparingly soluble salt , the product of Solubility (mol/lit) of all the…

Q: What mass (in g) of sodium formate, HCOONA, must be added to 10.0 L of a 0.483 Maqueous solution of…

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Q: Which statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium…

A: Hi! Thank you for the question As per the honor code, We’ll answer the first question since the…

Q: A chemistry graduate student is given 300.mL of a 1.10M hydrocyanic acid  (HCN) solution.…

A: The formula for the calculation of pH of the given buffer solution is given below.

Q: Suppose you need to prepare a buffer system with a pH = 5.30 in the laboratory. The available acids…

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Q: 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker.  After 22.04 mL of NaOH is added to the beaker,…

A: The balanced equation for the reaction between sodium hydroxide and sulfuric acid is as follows.…

Q: (a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer.   What is the pH of the buffer after…

A: A buffer solution is made up of weak acid or base with its conjugate base or acid respectively. pH…

Q: 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker.  After 17.65 mL of NaOH is added to the beaker,…

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Q: A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which…

A: Given,

Q: A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x 104) and…

A: An aqueous solution efficient to withstand the pH changes and comprising weak acid/base combined…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has: Concentration of NH4Cl/NH4+ = 0.182 M Concentration of NH3…

Q: A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution.…

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Q: A buffer consists of 0.50 M NaH₂PO₄ and 0.40 M Na₂HPO₄.Phosphoric acid is a triprotic acid…

A: A buffer solution is prepared by mixing a weak acid and its conjugate base in the aqueous medium.…

Q: Consider the titration of 100.0 mL of 0.200 mol/L ethanoic acid, HC2H3O2(aq) (Ka = 1.8 x 10-5), by…

A: Here 100 ml of 0.2M ethanoic acid is titrated with 150 ml of 0.1 M potassium hydroxide. We have to…

Q: Calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer…

A: Given- Concentration of CH3CH2NH2 = 0.2604 M Concentration of  CH3CH2NH3Cl = 0.2404 M Volume of…

Q: In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid…

A: Molarity gives the concentration of a solution. It gives the number of moles of the solute dissolved…

Q: A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of…

A: Moles of weak base ammonia = 0.713 mole Moles of conjugate acid (NH4+) = 0.603 mol  Moles of HNO3…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for