A buffer solution is to be made wherein the pH of the acetic acid (pKa = 4.74) buffer is 5.08. If 6.86 moles of acetate will be used, how much will be total moles of the entire buffer?

Q: A 1.34 L buffer solution consists of 0.174 M butanoic acid and 0.250 M sodium butanoate. Calculate…

A: The pH scale is given by the scientist Sorensen in order to express the [H3O+] ion of a solution. It…

Q: Methyl red has a pk, of 5.0 and is red in its acid form and yellow in its basic form. If several…

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Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: pH is the negative logarithm of concentration of H+ ion with base 10. pH=-log10H+ Where H+ is the…

Q: calculate the buffer capacity of a buffer consisiting 0.05 moles each of acetic acid and sodium…

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Q: What will be the total buffer concentration? What is the pH of a solution contains acetic acid d…

A: The solution which is made by the mixing of a weak acid and its conjugate base or vice verse is know…

Q: A buffer is prepared using lactic acid (HLac) and sodium lactose (NaLac). 0.300 dm3 of the 0.500…

A: Buffer solution - it is an aqueous solution consisting of the mixture of a weak acid and its…

Q: A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is…

A: According to Henderson-Hasselbalch equation,pH = pKa + log [conjugate base/acid]

Q: The pK, value for HF is 3.14. Would a buffer prepared from HF and NaF with a pH of 1.14 be…

A: “Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: calculate the ph of a 0.500l of a buffer solution composed of 0.50m formic acid and 0.70m sodium…

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Q: A buffer solution contains 0.457 M ammonium bromide and 0.335 M ammonia. If 0.0430 moles of sodium…

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Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of benzoic acid (pKa = 4.20) and…

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Q: An aqueous solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium…

A: Given: Buffer solution of hydrazoic acid i.e. HN3 and sodium azide i.e. NaN3.

Q: Report the largest pK for the weak acid whose titration curve is shown. PH [OH ]

A: The titration curve given is,

Q: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution…

A: Ammonia is a weak base and form a buffer solution with NH4Cl The pH of buffer is close to 9-10.…

Q: A 1.35 L buffer solution consists of 0.175 M butanoic acid and 0.336 M sodium butanoate. Calculate…

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Q: 4. How many grams of sodium lactate, NAC3H5O3, should be added to 1.0OL of 0.150M lactic acid,…

A: To calculate the grams of sodium lactate , we would use Henderson Hasselbalch equation.

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 solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium…

A: The pH does not decrease drastically because the HCl reacts with Chloroacetate in the buffer…

Q: A 1.40 L buffer solution consists of 0.256 M propanoic acid and 0.105 M sodium propanoate. Calculate…

A: This is an acidic buffer solution.  Moles of propanoic acid = .256*1.4 = 0.3584  Moles of sodium…

Q: When you prepare a buffer, it is recommended to use a weak acid whose pKa is close to the pH…

A: Here we have to explain why to make a buffer solution the weak acid chosen should have pKa close to…

Q: A 1.32 L buffer solution consists of 0.178 M butanoic acid and 0.349 M sodium butanoate. Calculate…

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Q: If equal volumes of 0.29 M acetic acid and 0.12 M sodium hydroxide are mixed, what is the pH of the…

A: Henderson–Hasselbalch equation, pH = pKa + log [salt]/[acid]

Q: A sodium hydrogen carbonate-sodium carbonate buffer with a pH of 9.40 is prepared. Determine the…

A: Given: The pH of the sodium hydrogen carbonate-sodium carbonate buffer = 9.40  We have to find the…

Q: Suggest 2 different buffer systems that can be used for the preparation of a pH=7.7 buffer solution?…

A: Buffer is such solution which makes pH of the solution constant.

Q: Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of formic acid (pKa=3.74) and 40.0…

A: Weak acid are those acid which does not dissociate completely in aqueous solution and weak base are…

Q: A 1.49 L buffer solution consists of 0.142 M butanoic acid and 0.286 M sodium butanoate. Calculate…

A: Given: Volume of buffer solution = 1.49 L The concentration of butanoic acid, (HA) = 0.142 M…

Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Given: pH = 5 Ka of acetic acid = 1.8×10-5   Calculation for pKa of the acetic acid: Calculation…

Q: 1.34 L buffer solution consists of 0.128 M butanoic acid and 0.289 M sodium butanoate. Calculate the…

A: When a strong base is added to the buffer solution, then it reacts with the weak acid of the buffer…

Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.127 M solution…

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Q: Methyl red has a pKa of 5.0 and is red in its acid form and yellow in its basic form. If several…

A: Methyl red is an indicator. In acidic medium, it turns into red colour and in basic medium it turns…

Q: Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is…

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Q: What is the pH of a buffer prepared by combining 0.441 moles of trimethylamine (a weak base) with…

A: Here we are required to find the pH of buffer solution of weak base and it's salt of conjugate acid

Q: 4. The molar ratio between a weak acid and its base conjugate was (3:2). Calculate the Ka of the…

A: Hendrson hasselbalch equation will be use to determine Ka value

Q: To produce a formate buffer solution that is at a pH of 4.06, what should the concentration of the…

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

Q: A buffer is made by adding solid sodium citrate (Na3C6H5O7) to a solution of 1.20 M-Na2HC6H5O7. The…

A: Na2HC6H5O7 is a weak acid with pKa value of approximately 6.39 Na3C6H5O7 is the conjugate base of…

Q: When the pH is below the pKa, is the buffer species more or less than 50% protonated? Explained in…

A: Given -> pH is below the pKa value.

Q: what is the mole ratio of ammonia to ammonium chloride in a buffer with a pH of 9.00?

A: The answer to the following question is-

Q: A buffer solution contains 0.285 M hydrofluoric acid and 0.326 M potassium fluoride. If 0.0252…

A: Given,  The molarity of Hydrofluoric acid = 0.285 M The molarity of Potassium fluoride = 0.326 M.…

Q: What must be the minimum concentration of cyanoacetic acid in 1.00L buffer solution of a pH 2.43…

A: Solution                     Given that Pka = 2.45 PH = 2.43 0.086 moles HCl is added Find…

Q: the pH of an acetate buffer prepared by dissolving sodium acetate (5.21 g) and acetic acid (2.19 g)

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Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Given, Concentration of lactic acid, [HLac] = 0.5 mol.dm-3 = 0.5 mol/L   (1 dm3 = 1 L) Volume of…

Q: What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer…

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Q: A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate…

A: Given- Volume of a buffer solution =1.5 0L Concentration of propanoic acid =0.280M  Concentration of…

Q: The pKa of the indicator methyl orange is 3.46. Over what pH range does this indicator change from…

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Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Given: pKa of lactic acid = 1.4 * 10-4

Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Given,Molarity of HLac=0.500mol.dm-3volume of HLac=0.300dm3Molarity of NaLac=0.300mol.dm-3volume of…

Q: Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 125 mL of a buffer hav- ing a…

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Q: How many moles of sodium acetate must be added to 2.0 L of 0.10 M acetic acid to give a solution…

A: Calculation of no. of mol of acetic acid: No. of mol=Molarity×Volume=0.10 mol/L×2.0 L=0.2 mol…