Consider a beaker containing 50 mL of 0.20 M of a weak acid (HA) with a pKa of 5.25.    How many mL of 0.20 M NaOH (a strong base) should be added to the beaker make a buffer with pH 5.83? How many mL of 0.20 M A- (the weak conjugate base of the weak acid, HA) should be added to the beaker make a buffer with pH 5.83?

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.30 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

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Q: What is the pH of the buffer made by adding 30.0 mL of 0.15 M HC2H3O2 ( acetic acid ) to 70 mL of…

A: Concentration of both acid and salt will changed if we add both because volume is increases.

Q: Calculate the pH of a buffer solution that contains 0.34M benzoic acid and 0.49 M potassium…

A: Using Henderson equation , we can solve this problem. Here benzoic acid is weak acid and potassium…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Introduction:  We have to calculate number of moles of NaOH . Given : pH = 3.70  Ka= 6.8 × 10-4

Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to  100.00 mL  of a 0.115 M solution…

A: Mass (in grams) of sodium acetate (CH3COONa) must be added to  100.00 mL of a 0.115 M solution of…

Q: The bicarbonate/ carbonic acid buffer is of extreme importance to our bodies. The pH of importance…

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Q: A student needs to prepare a buffer solution with a pH of 5.73. Assuming a pKa of 4.06, how many mL…

A: Given,Molarity of NaOH = 0.1 MMolarity of acid ( HB ) = 0.1 Mvolume of HB = 15.0 mLpH of the buffer…

Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

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Q: Calculate the pH of a buffer prepared by adding 0.44 moles of acetic acid and 0.25 moles of acetate…

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Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Write Henderson Hasselbalch equation, pH = pKa + log[base][acid] where Ka is the acid dissociation…

Q: Part A: A 252-mL buffer solution is 0.420 M in ammonia (NH3) and 0.303 M in ammonium chloride…

A: We would use Henderson Hasselbalch equation to calculate  initial pH.  Then , HBr which is a strong…

Q: A 1.33 L buffer solution consists of 0.263 M propanoic acid and 0.198 M sodium propanoate. Calculate…

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Q: calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 3.00 g…

A: Molarity of sodium benzoate can be calculated as follows:

Q: You are provided with 100 ml of 1 M HCl. You add a 1 ml of solution of 0.1M sodium acetate in water…

A: Let's analyze each option:The pH of the final solution does not change significantly:When we add 1…

Q: 2. How many ml of 0.2 M HCI needs to be added to 100.0 ml of 0.2 M Sodium acetate (kb for acetate is…

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

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Q: Calculate the pH of a buffer comprised of 0.10 M hypochlorous acid and 0.080 M sodium hypochlorite.…

A: Formula used:-  pH = pKa + log [salt]/[acid]

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: Recall the reaction that will occur here HF + NaOH→ NaF + H2OHere,we recall Henderson Hasselbalch…

Q: What concentration of sodium benzoate must be used to create a buffer solution with a pH of 5.63 if…

A: Use a udic buffer equation to get MOLARITY of sodium benzoate. Buffer mixture is defined as an…

Q: You need to prepare an acetate buffer of pH 5.45 from a 0.654 M acetic acid solution and a 2.53 M…

A: The number of moles of acetic acid (nAcOH) in 480 mL 0.654 M solution is calculated using equation…

Q: Solutions Solution A: Solution B: Solution C: Solution D: 0.565 M HOCI 0.376 M HC1O4 0.817 M HCO₂H…

A: Buffer solution: It is a solution that can resist changes in pH when small amounts of acid or base…

Q: An aqueous solution contains 0.449 M ethylamine (C₂H5NH₂). How many mL of 0.303 M perchloric acid…

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Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and…

A: Let y mL benzoic acid and (100 – y) mL sodium benzoate are mixed. For acidic buffer solution,  pH =…

Q: suppose that the ph of buffer A turned out at ph 5.5 instead of ph 5.0 (100.0 mL of a 0.5 M buffer)…

A: Buffer solution is defined as a solution which resists any change in its pH value even when small…

Q: What is the pH of a buffer made by combining 45.0 mL of 0.150 M nitrous acid and 20.0 mL of 0.175 M…

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Q: The concentration of H3O+H3⁢O+ in the buffer prepared in the previous question is 2.27×10−5…

A: Since, Negative logarithm of concentration of H+ ion is known as pH of the solution. i.e. pH =…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

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Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

A:

Q: You need to prepare an acetate buffer of pH 5.27 from a 0.895 M acetic acid solution and a 2.71 M…

A: Let volume of KOH = V Liter  Molarity of KOH = 2.71 M  So,  Number of moles of KOH = Molarity of KOH…

Q: Which of the following weak acids would be suitable for making a buffer at pH = 3.50? chlorous acid…

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Q: Lactate is an important component in some intravenous solutions. Given pKa = 3.86 for lactic acid,…

A: pH = pKa  +  log ( [ conjugate base ]/[weak acid] ) ---------(i) pKa = 3.86 ( given) HC3H5O3…

Q: An aqueous solution contains 0.430 M ammonia (NH3). How many mL of 0.384 M nitric acid would have to…

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Q: 20 An aqueous potassium iodate (KIO3) solution is made by dissolving 538 g of KIO3 in sufficient…

A: mass of KIO3 = 538 gvolume of the solution = 4.20 Lmolarity of the KIO3 solution = ?Note: molar mass…

Q: What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9?…

A: Since you have asked multiple question, as per our company guidelines we are supposed to answer the…

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A:

Q: pH

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Q: You are asked to make a buffer to a pH of 4.00 and you have the following acids to do it with (pKa…

A: Given , The pH of buffer = 4.00

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.