Answered: Calculate the pH after the addition of…

Science

Chemistry

Calculate the pH after the addition of 0.0050 mol of NaOH to the buffer in 9.1.4. (0.200 M NH4Cl - 0.200 M NH3 buffer)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

See similar textbooks

Related questions

Q: How would prepare 750ml of 0.1M NaCl, 0.5M Tris-HCl solution given that you have 5M NaCl and 1M…

A: Molarity is defined as the moles of solute present per liter of solution. For example: 5 M NaCl…

Q: cion 6 A 500.mL buffer solution is prepared by mixing 50. mL of 0.650 M NaOH and 45 mL 0.500 M…

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka=1.75X10°). Calculate the…

A: Given, Molarity of CH3COOH = 0.40 M Volume of buffer = 200.0 mL = 0.200 L Molarity of CH3COONa =…

Q: with

A: pH = pKa + log( salt / Acid ) pH = -log(Ka) + log ( [A-] / [HA] ) Where : pKa = -log(Ka) and salt…

Q: Assuming 0.10 M Na2HAsO4, 0.40 M NaOH and 0.50 M HCl solutions are available in your laboratory.…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid and 1.00 M in sodium acetate…

A: pKa value for acetic acid = 4.75

Q: 4. Calculate the change in pH that results from adding 25 mL of 0.010F HCI to 500ml buffer solution…

A: Given, [NH3] = 0.25 M [NH4Cl] = 0.15 M Volume of the buffer in mL = 500 mL Volume of HCl added =…

Q: Would a solution that contains equal volumes of 0.10 M NAOH and 0.20 M Na*CiO" (sodium hypochlorite)…

Q: A buffer is prepared by adding 0.300mol of NaF to 1.00 L of 0.200 M HF. Calculate the pH of the…

A: Moles of NaF =0.300 moleVolume of Buffer = 1 LConcentration of NaF ==Moles of NaFVolume of…

Q: Calculate the volume of 1.0 M NaOH that would cause 20ml of 1.0M acetic acid and 10ml of 1,0M sodium…

A: when a buffer lost their Buffering capacity it's means that, buffer is react with strong acid or…

Q: What mass of ammonium chloride should be added to 2.55 L of a 0.155 M NH3 in order to obtain a…

A: The pH of a buffer solution can be calculated by using Henderson- Hasselbalch equation.

Q: To make a buffer with a pH of 5.00, how much sodium acetate would you have to add to a solution that…

Q: grams

Q: -4 A chemistry graduate student is given 100. mL of a 1.50M trimethylamine (CH,),N)s solution.…

Q: 2. A solution is 0.10M in Mg(NO3)2. a. What conce ntration of OH is required to just start…

A: (a). Concentration of OH- required can be calculated as:

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: How much 10.0 M HNO3 m

Q: A buffer containing 0.2000 M of acid, HA, and 0.1500 M of its conjugate base, A⁻, has a pH of 3.35.…

Q: A buffer solution is 0.40 M in acetic acid and 0.38M sodium acetate (Ka= 1.75X105). Calculate the…

Q: A buffer system is prepared that is 0.020 M in NH3 and 0.030M in NH4*. What is the concentration, in…

Q: What amount of HCl gas must be added to 1.00 L of a buffer solution that contains [acetic acid] =…

A: Given,1.0L of a buffer solution that contains [acetic acid] = 2.0 M and [acetate] = 1.0 M .…

Q: What mass of ammonium chloride should be added to 2.45 L of a 0.150 M NH3 to obtain a buffer with a…

A: The given buffer solution is a mixture of weak base NH3 and its conjugate acid ammonium chloride…

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: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: The equation for neutralisation reaction between acetic acid and KOH is:

Q: How many grams of sodium acetate, NaC2H302, would have to be added to 1.0 L of 0.85 M acetic acid…

Q: Preparation of 40 mL of an acetate buffer (pH 4.2) 0.2 M acetic acid (pKa = 4.8) and 0.2 M sodium…

A: pH is used to get the acidic or alkaline values of a solution. A buffer solution is one which…

Q: Assuming 1.00 M Na2HAsO4, 2.00 M NaOH and 2.00 M HCl solutions are available in your laboratory.…

Q: How many mL of 4.50 M sodium hydroxide must be added to 250 mL of a 0.200 M nitrous acid solution to…

Q: A buffer solution is prepared by combining 3.00 grams of 3-nitrobenzoic acid (138.12g/mol) in…

A: (A) The molar mass of 3-nitrobenzoic acid is 167.12 g/mol. The moles of acid is calculated as…

Q: Calculate the pH of 0.500 L of a buffer solution composed of 1.50 M citric acid and 0.75 M sodium…

A: The Henderson-Hasselbalch equation gives a relationship between the pH of acids and their acid…

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka= 1.75X10). Calculate the…

A: As HCl is strong acid , when it's added to the buffer solution the conjugate base present in the…

Q: Shown in the graph below is the titration curve that results when 25.0mL 0.200M HClO is titrated…

A: a) Titration curve of a strong acid (HclO4) and strong base is shown below

Q: Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing…

A: Frist determine pKa value from given Ka value. pKa=-log Ka=-log 2.9×10-8=7.54 Now determine the…

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: 6. If 25.1 mL of 0.109M acid with a pKa of 5.27 is titrated with 0.108 M NaOH solution, what is the…

A: The volume of acid V1=25.1 mL The concentration of acid C1=0.109 M The strength of an acid is pKa =…

Q: To make a buffer with a pH of 5.00, how much sodium acetate would you have to add to a solution that…

A: Given: pH= 5.00 Moles of acetic acid= 10.0 mmol

Q: How many milliliters of 0.105 M HCl should be added to 200.0 mL of 0.010 9 M triethylamine to give a…

Q: Acetic acid’s pKa is 4.75 and nitrous acid’s pKa is 3.16. If you made one buffer of equal parts…

A: Given: pKa of acetic acid = 4.75 pKa of nitrous acid = 3.16 And both the buffers have an equal…

Q: have to be added to 1.0 L of a 1.948 M HA solution in order to obtain a buffer of 3.11? (The Ka for…

A: We will use buffer equation

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka= 1.75X10). Calculate the…

Q: If you have 0.20 M acetic acid and 0.20 M sodium acetate, how can you make a buffer with pH about…

Q: What mass in unit of gram of solid NaHCO3 (molar mass = 84.00 g/mol) should be added to 1.00 L of…

A: In this question, we want to determine the mass of NaHCO3. How we can determine, you can see…

Q: Calculate the change in pH after adding (2 g) from NaOH and molecular weight (40 g/mol) to a liter…

A: The change in pH after addition of base has to be calculated.

Q: 6. "How many grams of HCI would need to be added to 25.0 ml of a 0.20 M solution of NaCICH₂CO₂ in…

A: Given, Molarity of NaClCH2COO = 0.20 M Volume of NaClCH2COO in mL = 25.0 mL pH of the buffer =…

Q: In the lab, you have the following chemicals available to you: 1.00M H3PO4, NaHzPO49), NazHPO4(9),…

Q: What is the pH of a buffer that is 0.120 M in HA and 0.080 M in KA? For HA, K, = 1.8x104.

A: To solve this problem we will use Henderson - Hasselbalch equation of weak acid and it's conjugated…

Q: 2) Calculate how you would prepare 1.000 / of a pH 9.50 buffer made from NH3 and NH,CI. You are…

Q: What mass of sodium benzoate should you add to 150.0 mL of a 0.15 M benzoic acid solution to obtain…

A: The mass of sodium benzoate that should be added to 150.0 mL of a 0.15 M benzoic acid solution in…

Q: Find the pH of a buffer that consists of 0.12 M boric acid(H₃BO₃) and 0.82 M sodium borate (NaH₂BO₃)…

A: The Henderson - Hasselbalch equation is an important method which is used for the calculation of the…

Q: Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing…

Concept explainers

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.

Question

Calculate the pH after the addition of 0.0050 mol of NaOH to the buffer in 9.1.4. (0.200 M NH₄Cl - 0.200 M NH₃ buffer)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Calculate the pH of the buffer prepared by mixing 2.00 g of NaOH with 12.0 g NH4Cl and diluting to 500 mL with water.
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 solution is 5.881. The dissociation constant Ka of HA is 5.66×10−7 A. What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. B. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
a. 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 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10^−7. b. What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. c. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
A buffer was prepared by mixing 50.0mL of 0.10 M HX and 25.0mL of 0.10 M NaOH. The Ka of HX is 1.5x10-6. Calculate the pH of this buffer using a NICE table.
What mass of sodium benzoate should you add to 150.0 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25? (Assume no volume change.)
part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What would be the pH of this solution? part b: How many milliliters (mL) of 19.00 M NaOH are need to adjust the pH of this buffer to pH 10.00? Please answer part b
A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH of the resulting solution after 0.0750 mol of HCl are added to 250. mL of the buffer? Assume that the change in volume is negligible. Enter your response in pH units to the nearest 0.1.
4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.22 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH)
How many g of sodium nitrate (NaNO2, 100% ionized in water) do you need to add to 4.00L of 0.500M nitrous acid to make a buffer of 3.20 pH. The Ka of nitrous acid is 4.6 x 10-4. Assume the sodium nitrite will not increase the volume of the solution.