What is the pH of a buffer solution that is 0.20 M propionic acid and 0.46 M sodium propionate?

Q: If a buffer is present at a pH of 4.8 and the buffer is then diluted, does the pH of the buffer…

A: If a buffer is present at a pH of 4.8 and the buffer is then diluted, the concentration changes. But…

Q: What is the final pH value of a buffer if 1 ml of hydrochloric acid (1 N) is added into 50 ml of…

A: 1-First calculate the mmoles of hydrochloric acid.  For HCl, 1N is equal to 1M ( normality =…

Q: An aqueous solution contains 0.370 M nitrous acid. How many mL of 0.236 M potassium hydroxide would…

A: Solution: We know nitrous acid (HNO2) is a weak acid and KOH is the strong base. So they can form…

Q: An aqueous solution is prepared to be 0.232 M in sodium nitrite and 0.101 M in acetic acid. (1) Is…

A: An aqueous solution is prepared to be 0.232 M in sodium nitrite and 0.101 M in acetic acid. 1) Is…

Q: When a 20.6 mL sample of a 0.423 M aqueous acetic acid solution is titrated with a 0.436 M aqueous…

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Q: A buffer solution contains 0.371 Mhydrocyanic acid and 0.449 M potassium cyanide. If 0.0218 moles of…

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

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction between the sodium hydroxide and hypochlorous acid as shown below. At standard…

Q: An aqueous solution is prepared to be 0.221 M in sodium formate and 0.113 M in benzoic acid. (1) Is…

A: Solution:   (1):   Yes, it is a buffer solution. (2nd) and (3rd) part are solved in step no. 2 which…

Q: A buffer solution is 0.453 M in KH2PO4 and 0.271 M in K2HPO4. If Ka for H2PO4- is 6.2x10^-8, what is…

A: Buffer solutions show resistance to change its pH upon addition of strong acids or bases, which is a…

Q: A 36.0 ml. sample of a 0.446 M aqueous hypochlorous acid solution is titrated with a 0.205 M aqueous…

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Q: How does the buffer solution absorb the added H+ and OH- to make the pH change very small?

A: A buffer can be acidic or basic in nature. A buffer that contains a weak acid with its conjugate…

Q: what is the ph of a buffer solution composed of 0.50m formic acid and 0.70m sodium formate

A: Answer: 3.90  Given buffer solution contains formic acid,  HCOOH , a weak acid, and sodium formate,…

Q: Calculate the pH of a 0.100 M Na3PO4 solution. Find the mL of 0.40 M HClO4 that must be added to 100…

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Q: When a 19.4 mL sample of a 0.395 M aqueous acetic acid solution is titrated with a 0.345 M aqueous…

A: Given, Volume of acetic acid = 19.4 mL Concentration of acetic acid = 0.395 M Volume of KOH = 33.3…

Q: If a buffer solution is 0.200 M in a weak base (Kb=7.4×10−5) and 0.450 M in its conjugate acid, what…

A: Calculate the pOH value of the given buffer solution,            pKb = - log Kb = -log (7.4 × 10-5)…

Q: If a buffer solution is 0.290 M in a weak base (K, = 1.4 × 10-5) and 0.580 M in its conjugate acid,…

A: pH of the buffer solution is determined by the Henderson-Hasselbalch equation as shown below: pH =…

Q: Which of the following combination will result in a buffered solution? O 0.1 M sodium acetate and…

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Q: When a 20.6 mL sample of a 0.394 M aqueous hypochlorous acid solution is titrated with a 0.328 M…

A: volume of HClO = 20.6 mL = 0.0206 L  Molarity of HClO = 0.394 M Molarity of  NaOH = 0.328 M For…

Q: A buffer solution contains 0.209 M ammonium chloride and 0.301 M ammonia. If 0.0515 moles of…

A: 1- First calculate the moles of salt and base before addition of acid HI :  a) moles of NH4Cl = […

Q: An aqueous solution contains 0.339 M nitrous acid. How many mL of 0.370 M sodium hydroxide would…

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Q: What is the pH of a buffer solution containing 0.25 M acetic acid and 0.030 M sodium acetate?

A: The pKa of acetic acid=4.76 Given: The concentration of acetic acid [CH3COOH]=0.25 M  The…

Q: An aqueous solution contains 0.494 M ethylamine (C2H5NH2). How many mL of 0.206 M hydroiodic acid…

A: Given data,Molarity of ethylamine=0.494MMolarity of HI=0.206MVolume of buffer=225mL=0.225LpH=10.6…

Q: what is the pH

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Q: When a 19.3 mL sample of a 0.316 M aqueous acetic acid solution is titrated with a 0.448 M aqueous…

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Q: WHAT IS THE PH OF A SOLUTION THAT IS 0.40 M IN SODIUM ACETATE.....

A: Bronsted –Lowry conjugate acid-Base pairs:When an acid is dissolved in water, the acid donates a…

Q: Calculate the pH of a buffer solution that is 2.00 M in phosphoric acid and 1.50 M in potassium…

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Q: If a buffer solution is 0.250 M in a weak acid (?a=2.3×10^−5) and 0.440 M in its conjugate base,…

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Q: How many moles of potassium hydroxide would have to be added to 225 mL of a 0.478 M acetic acid…

A: Here KOH was added in acetic acid. pKa of acetic acid is 4.75 Now, 225mL 0.478M CH3COOH =…

Q: What is the function of a buffer solution?

A: A buffer is a solution that can resist pH change upon the addition of an acidic or basic components.…

Q: A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH…

A: The pH of the buffer solution is find out using the Henderson-Hasselbalch equation. This equation…

Q: If a buffer solution is made from 300.0 mL of 1.6 M aniline salt mixed with 250.0 mL of 2.0 M…

A: Given: Concentration of aniline salt = 1.6 M Concentration of aniline = 2.0 M Volume of aniline salt…

Q: An aqueous solution contains 0.396 M ethylamine (C2H5NH2). How many mL of 0.268 M perchloric acid…

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Q: A buffer solution is desired to be prepared by mixing 100 mL of 0.6M ammonia solution and 150 mL of…

A: Given, Volume of ammonia = 100 mL Molarity of ammonia = 0.6 M Volume of ammonium chloride = 150 mL…

Q: There are 250 ml of a Buffer solution, where the concentration is 0.225 M of acetate of sodium and…

A: Buffer solution is a mixture of weak acid and it's conjugate base or a weak base with its conjugate…

Q: Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.

A: The Henderson hasselbalch equation for calculation of pH of a buffer is pH = pKa + log[base][acid]…

Q: An aqueous solution contains 0.329 M methylamine (CH3NH2). How many mL of 0.305 M perchloric acid…

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Q: The pH of a buffer is higher than the pH at which it would have the greatest buffering capacity in…

A: Buffer solution is a solution of weak acid and conjugate base OR weak base and conjugate acid which…

Q: An aqueous solution contains 0.484 M methylamine (CH3NH2). How many mL of 0.388 M perchloric acid…

A:

Q: If a buffer solution is 0.180 M in a weak base (Kb=7.5×10−5) and 0.400 M in its conjugate acid, what…

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Q: When a 22.9 ml. sample of a 0.338 M aqueous hypochlorous acid solution is titrated with a 0.367 M…

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Q: How does chemical equilibrium work to moderate pH? What happens when you add a strong acid to the…

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Q: What is an acid-base buffer and what two components must be present? What important value do…

A: Buffer Solution is a water-based solution or aqueous solution that consists of a mixture of a weak…

Q: An aqueous solution contains 0.305 M methylamine (CH3NH2). How many mL of 0.365 M hydroiodic acid…

A: Interpretation-  To determine the volume ( mL) of 0.365 M hydroiodic acid would have to be added to…

Q: What is the pH of a buffer solution that is 0.24M NH3 and 0.20M NH4Cl?

A: Given,Concentration of NH3 = 0.24 MConcentration of NH4Cl = 0.20 MAmmonia (NH3), is a weak base with…

Q: An aqueous solution is prepared to be 0.405 M in sodium fluoride and 0.261 M in acetic acid . (1) Is…

A: Given 0.405 M in sodium fluoride and 0.261 M in acetic acid . Add HBr 0.133 moles in 1L solution

Q: When a 27.5 mL sample of a 0.323 M aqueous hypochlorous acid solution is titrated with a 0.484 M…

A: Since both acid and base are strong in nature hence they both will react immediately. Since moles of…

Q: How many moles of sodium hydroxide would have to be added to 225 mL of a 0.332 M hydrocyanic acid…

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Q: a. Suppose a solution contains 0.50 M NaHPO4 and 0.80 M NazHPO4. What pH should be expected for this…

A: Recall Henderson Hasselbalch equation to calculate pH of the given buffer solution          pH=pKa +…

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.