How many grams of sodium acetate (82.03 g/mol) should you add to 250 mL of 0.100 M acetic acid (Ka = 1.8 x10-5) to create a buffer at pH 4.40?

Q: 1. Why was it important to use "flat" soft drinks for your titrations? Would your calculations of…

A: Here we are titrating soft drink which contains acids with strong base, NaOH to find the citric acid…

Q: A buffer is made using 100.0 mL of 0.200 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M…

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Q: 40. If you add 8.0 mL of 0.10 M HCl to 25 mL lactic acid/lactate buffer that is 0.10 M lactic acid…

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Q: Suppose a solution contains a mixture of 0.15 M methamphetamine (pKb = 4.50) and 0.31 M…

A: Given:pKa = 9.50pKb = 4.500.15 M methamphetamine0.31 M methamphetamine hydrochlorideThe given…

Q: A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid.  You…

A: Buffer is a substance which resists or very small change in the pH value of the solution when the…

Q: Consider the titration of a 40.0 mL of 0.189 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH. How…

A: The halfway point of the titration is that point where half of the acids has been reacted. The…

Q: Suppose you have 100 mL of a buffer containing 0.100 M acetic acid and 0.0500 M sodium acetate.…

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: Consider a 1.0 L buffer containing 0.086 mol L- CH3COOH and 0.082 mol L-1 CH3COO™. What is the pH of…

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Q: Suppose you have 150 mL of a buffer containing 0.100 M acetic acid and 0.0500 M sodium acetate.…

A: Given,  Volume of the buffer = 150 mL  Molarity of CH3COOH = 0.100 M Molarity of CH3COONa = 0.0500 M…

Q: Does the 0.100 came from the conversion of 100 mL? Or is it from the given 0.100 M buffer?

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Q: Consider a 1.0 L buffer containing 0.11 mol L-1 HF and 0.11 mol L-1 F-. What is the pH of the…

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Q: How does the buffer react to the addition of acids and bases? In comparison, how does water react to…

A: Buffer solutions are aqueous solutions that resist the change in pH on addition of small amount of…

Q: A 30.0 mL sample of 0.165 M propanoic acid (Ka = 1.3x10^-5) is titrated with 0.300 M KOH. Calculate…

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Q: 2. How many grams of sodium acetate is needed to add to a 0.2M acetic acid to prepare a buffer of…

A: Concentration of acetic acid = 0.2M pH of buffer solution to be prepared = 5

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: What is the pH of a buffer prepared by combining 0.36 moles of a weak acid, HA, with 0.69 moles of…

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Q: How many grams of sodium hypochlorite, NACIO, need to be added to 227 mL of a 0.185 M solution of…

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Q: Calculate the pH during the titration with NaOH after addition of: a. 50 mL of 0.1 mol L-1 NaOH to…

A: Solution: We know that acid-base titration method is most used traditional method to calculate…

Q: Calculate the pH of the buffer prepared by mixing 2.00 g of NaOH with 12.0 g NH4Cl and diluting to…

A: A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution…

Q: 4. Methanoic acid, HCOOH, has a K₂ value of 1.58 x 104 mol/L. What ratio of methanoic acid and…

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Q: grams

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Q: A 44.20 mL sample of phenol (Ka=1.60x10-10) analyte with a concentration of 0.113 mol L-1 is…

A: We have to calculate the pH at equivalence point.

Q: 2.Calculate the pH of the buffer prepared by mixing 2.00 g of NaOH with 7.50 g of disodium hydrogen…

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution. The…

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…

A: Given-> Volume of NH3 = 50.0 ml Molarity of NH3 = 0.15 M Volume of HCl = 15.0 ml Molarity of HCl…

Q: If you add 5.0 mL of 0.20 M HCI to 25 mL lactic acid/lactate buffer that is 0.10 M lactic acid and…

A: The pH of a buffer solution is determined by Henderson equation…

Q: If you wanted to make 1.30 L of a solution of 80.0 mM acetate buffer at a pH of 5.20. How many moles…

A: We can use Henderson's Hasselbalch equation to solve this problem. That is, pH = pka + log…

Q: How many grams of solid KF (molar mass = 58 g/mol) should be added to 1.00 L of 0.1 M HF to make a…

A: HF is a weak acid. KF is a salt made up of weak acid HF and strong base KOH.  Henderson equation for…

Q: How much solid sodium acetate (CH3COONa) is needed to prepare a buffer solution at ph 5 if you have…

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Q: 3.28 g of sodium acetate (82 g/mol) added to 400 mL of acetic acid to produce a buffer solution that…

A: Given 3.28 g of sodium acetate added to 400 ml of acetic acid to make buffer of pH =5 and pKa of…

Q: How many grams of Na2CO3 must you add to 1.5 L of freshly prepared 0.2 M NaHCO3 to make the buffer…

A: Given,  Volume of the buffer in L = 1.5 L  Molarity of NaHCO3 or HCO3- = 0.2 M  pH of the buffer =…

Q: What volume of 0.110 M Hydrochloric acid needs to be added to 30 mL of 0.100 M ammonia to make a…

A: We know the Henderson-Hasselback equation is, pH=pKa +salt/acid Given Value;   The concentration of…

Q: What is the pH of the buffer solution that contains 2.1 g of NH4Cl in 250 mL of 0.12 M NH3? Is the…

A: Buffer solutions are designated as alkaline buffer solutions and acidic buffer solutions. Given…

Q: The 100. mL of buffer solution contains 0.08 M benzonic acid and 0.06 M sodium benzoate. What is the…

A: here we are required to find the pH of buffer

Q: a)  What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x 105)…

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Q: A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein end point with 25.0 mL…

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Q: 5) You need to make 250.0 mL of a buffer with a pH of 4.10, in the chemical storage room you found…

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Q: You are making a buffer solution in the lab by combining the weak acid H2PO4- with its conjugate…

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Q: What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA in…

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Q: Solve this?

A: pH = 9.2 pH + pOH = 14 pOH = 14-9.2 = 4.8

Q: When 100 mL of a 1.0M strong acid is 50% titrated with 1.0M strong base, the volume of the base…

A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: What is the pH of  a buffer containing 250 mmoles of HCOOH (Ka = 1.8 x 10-4) and 482 mmoles of KHCOO…

A: The reaction between the sodium hydroxide (NaOH) and formic acid (HCOOH) as shown below. In this…

Q: Calculate. If you have 150 ml of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric…

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Q: 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH…

A: Volume of solution = 50.0ml  Volume of NaOH = 8.55 ml

Q: How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH =…

A: We have given that pH = 5.0 Ka = 1.8×10-5 Pka = -log(1.8×10-5) = 4.74 Concentration of Acetic Acid =…

Q: Zane titrated 25.0 mL of 0.40 M propioic acid with 0.20 M NaOH. What volume of NaOH is needed to…

A: we have to calculate the volume of NaOH for equivalence point

Q: What mass (in g) of ammonium chloride (NH4Cl) should be added to 2.60 L of a 0.155 M NH3 to obtain a…

A: Buffer solution is made of weak acid or base and their corresponding conjugate base or acid…

Q: Calculate the pH of the buffer prepared by mixing 2.00 g of NaOH with 80.0 mmol of salicylic acid…

A: This question is related to finding out the pH of the given buffer solution. Follow step-by-step

Q: Consider the titration of a 25.0mL sample of 0.195M acetic acid (CH3COOH) with 0.300M NaOH. How many…

A: During titration, the point at which the moles of added titrant becomes equivalent to moles of that…

Q: Methanoic acid, HCOOH, has a K₂ value of 1.58 x 104 mol/L. What ratio of methanoic acid and sodium…

A: Consider the given information is as follows; Ka of HCOOH = 1.58×10-4 mol/L pH = 4 Methnoic…

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.