A chemist creates 0.375 L of a 0.18 M acetic acid (CH3COOH) and 0.29 M sodium acetate (CH3COONa) buffer.  Note that the Ka of acetic acid is 1.8 x 10-5.   (a)  Write the chemical equation for how the buffer responds to the addition of HBr. (b)  What is the final pH if 0.0060 mol of HBr are added to the buffer solution

Q: A 50.0 mL sample of 0.100 M NH, is titrated with 0.100 M HBr. What is the most likely pH of the…

A: Answer :- 2.041  pH = 2.041…

Q: buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium…

A: The solution is as follows:

Q: A buffer solution contains 0.275 M of acetic acid, HC2 H 3 O 2 , and 0.350 M of its conjugate salt,…

A: Given : Concentration of HC2H3O2 = 0.275 M Concentration of KC2H3O2 = 0.350 M

Q: A buffer solution contains 0.753 M KClO2 (Ka = 1.1 x 10-2) and 0.659 M HClO2. If 0.244 moles of NaOH…

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Q: The Kp of lead(Il) hydroxide, Pb(OH)2, is 1.43 x 10-20 Calculate the molar solubility, s, of this…

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Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

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Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

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Q: A buffer solution contains 0.420 M NaHCO3 and 0.262 M Na2CO3. If 0.0303 moles of potassium hydroxide…

A: Initially, the solution contains a weak acid (NaHCO3) and its salt with a strong base (Na2CO3).…

Q: Choose the acid below that would make the most effective buffer for a solution to maintain a pH of…

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Q: A solution is prepared by dissolving 0.23 mol of lactic acid and 0.27 mol of sodium lactate in water…

A: The hydrochloric acid reacts with lactate ion present in the buffer solution to form lactic acid…

Q: A buffer solution is made up of 0.90 M formic acid and 0.90 M sodium formate. The formic acid has a…

A: Given : Concentration of formic acid = 0.90 M Concentration of sodium formate = 0.90 M Comcentration…

Q: Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong…

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Q: A buffer solution contains 1.250 mol of phenol, C6H5OH, and 0.950 mol of sodium phenoxide, C6H5ONa,…

A:

Q: A buffer solution contains 0.275 M of acetic acid, HC2 H 3 O 2 , and 0.350 M of its conjugate salt,…

A: Given : Concentration of HC2H3O2 = 0.275 M Concentration of KC2H3O2 = 0.350 M

Q: A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka  of the acetic acid is…

A: Calculation of pKa of acetic acid: pKa=-log Ka=-log (1.8×10-5)=4.745

Q: 4. The value of the solubility product, K for calcium hydroxide, Ca(OH), is 5.5 x 10, at25°C. (a)…

A: Given data:  Solubility product K sp Ca(OH)2= 5.5 x 10-6 Temperature = 250C

Q: Silver chromate, Ag2CrO4, is an "insoluble" substance with a Ksp value of 1.2 x 10^-12. Silver ion…

A: a. Let 's' be the molar solubility of Ag2Cro4 then,                 2s            s…

Q: Complete the ICE table below to show the change occurring and calculate the equilibrium for the…

A: The equilibrium reaction occurring between A- and HA just after the addition of hydrogen ions is…

Q: The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C.  Write a…

A:

Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given: The concentration of acetic acid is 0.100M. The volume of acetic acid is 100 mL. The…

Q: A buffer consists of 0.21 M H3PO4 and 0.38 M NaH2PO4. Given that the K values for H3PO4 are, Ka1 =…

A: Given that, a buffer is made by 0.21 M of H3PO4 and 0.38 M of NaH2PO4. The dissociation constant…

Q: Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can…

A: Initial number of moles of NaOH, acetic acid and sodium acetate is determined as follows, 1 mL =…

Q: Consider an acetate buffer system (Ka = 1.82 x 10 ). The buffer solution contains 0.200 M acetic…

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Q: If a buffer solution contains 1.6 M acetic acid and 2.3 M sodium acetate, what is the pH of the…

A: Given  ka (Ionisation constant)                 = 1.8 × 10-5 Concentration of CH3COOH         = 1.6…

Q: Consider an acetate buffer system (Ka = 1.82 x 105). The buffer solution contains 0.200 M acetic…

A: Given, Ka = 1.82× 10-5 concentration of acetic acid, [CH3COOH] = 0.200M concentration of sodium…

Q: A buffer solution is made that is 0.399 M in H2CO3 and 0.399 M in NaHCO3. If Ka1 for H2CO3 is 4.20 x…

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Q: a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M…

A: ICE table for the buffer solution of HNO2 and NaNO2 which will be produced after the addition of…

Q: The pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of…

A: Given,  The pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of NaA in…

Q: What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in…

A: Solution -

Q: An acetic acid buffer contains 0.6 M CH3COOH and 0.6 M CH3COONA. (CH3COOH has a K, 1.76 x 105.) What…

A: Given- Concentration of CH3COOH= 0.6M Concentration of CH3COONa= 0.6M Ka of CH3COOH=1.76 ×10 -5…

Q: The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: Describe the effect of pH on the solubility of Fe(OH)3

A: A reaction is said to be in equilibrium if the rate of the forward reaction is equal to the rate of…

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: Calcium hydroxide (Ca(OH)a) is a strong base. Its solubility is about 0.74 g/L at 25°C. 1. For a…

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Q: A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution.…

A: We have to calculate the mass of salt added.

Q: A buffer solution is composed of 1.923 g of KH,PO4 and 4.699 g of Naz HPO4. (K, for dihydrogen…

A: The pH of this buffer solution would be calculated using Henderson-Hassalbalch equation .

Q: A phenol/phenolate buffer was made up by mixing 0.0125 mol of phenol (C6H5OH) and 0.0135 m of…

A: Given : Moles of phenol = 0.0125 mol Moles of phenolate = 0.0135 mol Volume of buffer = 500 mL = 500…

Q: A 1.43 L buffer solution consists of 0.179 M butanoic acid and 0.300 M sodium butanoate. Calculate…

A: The pH of an acidic buffer can be calculated by using Henderson equation pH = pka + log10…

Q: 10. A buffer solution is made of mixture of aqueous methanolic acid, HCOOH. With aqueous sodium…

A: The solution that resists the change in pH is known as a buffer solution. The buffer solution is an…

Q: Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can…

A: Initial number of moles of NaOH, acetic acid and sodium acetate is determined as follows, 1 mL =…

Q: What is the pH of the buffer that results when 3,06 g of NagHPO, and 2.17 g of NaH,PO, are diluted…

A: Mass of Na2HPO4 = 3.06 g Mass of NaH2PO4 = 2.17 g Volume of buffer solution = 0.3 L Ka of H2PO4- =…

Q: A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given : Mass of CH3COONa = 1.000 g Volume of acetic acid solution = 100.00 mL = 0.100 L…

Q: 3. A formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and sodium formate…

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Q: A buffer solution contains 0.63 mol of hydrosulfuric acid (H,S) and 0.42 mol of sodium hydrogen…

A:

Q: A 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate…

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Q: A chemist added 0.15 mol of NaOH to a 1.00 L buffer that contained 0.50 M propanoic acid HC3H5O2)…

A:

Q: ou want to prepare 1.00 L of a buffer solution with a pH of 3.5.  You are given an 0.45 M solution…

A: pH =Pka + log[salt][acid][salt]=0.68yx+y=0.68y[acid]=0.45x-0.68yx+y[acid]=0.45-1.13ysubstititing the…

Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…

A: 1- First calculate the concentration of NaClO :  Using the Henderson equation,  pH = pKa +…

Q: Calculate the pH of the resulting solution when 100 mL of 0.5 M NH3, 50 mL of 0.3M HBr, 50 mL of…

A: