Answered: The mixture of 100.0 mL of 0.100 M NaOH…

The mixture of 100.0 mL of 0.100 M NaOH (aq) and 100.0 mL of 0.300 M CH3COOH (aq) will result in a buffer. (a) Explain why the resulting solution is a buffer. (b) What is the pH of this buffer?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 14QAP: A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to...

See similar textbooks

Related questions

Q: The solubility of Mg(OH)2 in a particular buffer solution is 0.66 g/L. Part APart complete What must…

A: Solubility product(Ksp) Solubility product is the concentration equilibrium of the saturated…

Q: A 10.00mL sample of 0.15 M of chlorous acid, HClO2 (aq) is titrated with 0.20 M sodium hydroxide,…

A: The dissociation of Chlorous acid (HClO2) is represented as:HClO2 (aq) ⇌ H+ (aq) + ClO2- (aq)Ka =…

Q: Calculate K.

A: We know that If the equilibrium constant is kc for forward reaction and the equilibrium constant is…

Q: A 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid. After…

A: The reaction will be as follows: HI(aq) + CH3NH2 ---------> CH3NH3+(aq) + I-(aq). The volume of…

Q: Sketch reasonably accurately the pH curve for the titration of 25.0 cm3 of 0.15 M Ba(OH)2(aq) with…

A: Initial pH will be according to the concentration of Ba (OH) 2. 1 mole Ba (OH) 2 have = 2 moles of…

Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…

A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…

Q: Group III (Al3+, Cr3+, Fe3+, Zn2+) cations produce very soluble sulphides so they can be…

A: The Group III cations include Al3+, Cr3+, Fe3+, Zn2+, Ni2+, Co2+ and Mn2+ ions. The solubility of…

Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

Q: A 28.4 mL sample of 0.366 M ethylamine, C2H5NH2, is titrated with 0.395 M hydrobromic acid. After…

Q: A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36)…

A: PH+Poh=14. This is basic buffer equation Poh=pkb+log[salt]/base Use this equation and get the…

Q: A buffer, consisting of H2PO4- and HPO42-, helps control the pH of physiological fluids. Many…

A: The mass of NaH2PO4 is 6.5 g. The mass of Na2HPO4 is 8.0g. The Volume of the solution is 355 mL. We…

Q: Choose the acid below that would make the most effective buffer for a solution to maintain a pH of…

Q: Calculate the molar solubility of iron(II) hydroxide in an aqueous solution buffered at pH = 6.07.

Q: The temperature for each solution is carried out at approximately 297 K where K w =1.00×10 −14 0.85…

A: Given, Kw = 1.00*10-14. Mass of HCl = 0.85g. Volume of solution = 5.5L. Moles and molarity of HCl…

Q: Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq.,…

A: The moles of hydrazoic acid HN3 are0.500 mol HN31 L×1 L1000 mL×50.00 mL=0.025 mol NH3 the…

Q: A solution is formed by adding 5.20 grams of solid potassium acetate, KC₂H₃O₂, to 500.0 ml of…

A: pH is negative logarithm of Hydrogen ion concentration

Q: A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which…

A: Given: Volume of buffer = 250.0 mL. Concentration of weak acid available = 0.51 M Concentration of…

Q: Calculate the molar solubility of Ag₂CrO₄.

A: Let molar solubility of Ag₂CrO4 is S

Q: What is the definition of titer? Specifically in analytical chemistry.

A: Explained as follows

Q: What is the pH of a boric acid buffer solution containing 0.25 mol/L of boric acid, H3BO3, and 0.50…

Q: A solution is formed by adding 3.20 grams of solid sodium hypochlorite, NaClO, to 500.0 ml of…

A: Answer: Solution will be basic due to hydrolysis of hypochlorite ion because it is the conjugate…

Q: A 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid. After…

A: This question can be solved using Henderson-Hesselbech equation as:

Q: A volume of 500.0 mL of 0.130 M NaOH is added to 555 mL of 0.250 M weak acid (Ka = 3.04 × 10¬³).…

A: Formula: pH = pKa + log[salt]/[acid] pKa = -logKa Number of mmoles = Molarity x volume (mL)

Q: The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:

Q: 2.60 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M…

Q: Determine the pH of a buffer system that is 1.00 M CH3COOH (aq) and 1.00 M CH3COONa (aq). LOHO

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

Q: A volume of 500.0 mL of 0.110 M NaOH is added to 525 mL of 0.250 M weak acid (Ka = 2.53 × 10-').…

A: Concentration of NaOH=0.11M Volume of NaOH=500 mL Volume of weak acid=525 mL Concentration of…

Q: A volume of 500.0 mL of 0.140 M NAOH is added to 565 mL of 0.250M weak acid (K = 6.60 x 10-). What…

A: Weak acid are those which does not dissociate completely in aqueous solution. pH of buffer solution…

Q: What is the molar solubility of silver chloride in 0.65 M NH3(aq)? Solubility

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

Q: Consider an acetate buffer system (Ka = 1.82 x 105). The buffer solution contains 0.200 M acetic…

A: Given, Ka = 1.82× 10-5 concentration of acetic acid, [CH3COOH] = 0.200M concentration of sodium…

Q: A volume of 500.0 mL of 0.160 M NAOH is added to 545 mL of 0.200 M weak acid (Ka = 6.62 x 10-). What…

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

Q: What are buffers in terms of acid-base equilibria, give an example, and can a buffer capacity be…

A: Buffer solution is a solution that is maintaining it's hydrogen ion concentration pH. With only…

Q: A 5.00 mL solution of H,SO4 was transferred to a 25.00 mL volumetric flask and was diluted to the…

Q: A stainless steel alloy is to be analyzed for its chromium content. A 3.30 g sample of the steel is…

A: Given Mass of sample steel = 3.30 g volume of solution = 250 ml Mass of BaCrO4 = 0.145 g M.m (molar…

Q: What is the correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 ?

Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…

Q: What is the pH of a buffer containing .11 M HCIO (aq) and .57 M NaCIO (aq)?

Q: 100.0 mL 0.15 M aqueous HF (K₁ = 6.8 x 104) is mixed with 125.0 mL 0.23 M NaF. What is the pH of the…

Q: A 0.040 M NaCH3CO2 aqueous solution is mixed with a 0.080 M CH3COOH aqueous solution, where the pKa…

A: Given data is as follows: The concentration of NaCH3CO2=NaCH3CO2= 0.040 M The concentration of…

Q: A 29.5 mL sample of 0.258 M ethylamine, C2H5NH2, is titrated with 0.340 M hydrochloric acid. After…

A: Given- Volume of ethylamine=29.5mL Concentration of ethylamine =0.258M Volume of hydrochloric acid=…

Q: The following reaction occurs: HNO,(aq) + NaOH(aq) → NaNO,(aq) + 2 H,0(1) Identify the correct…

A: When strong acid react with strong base neutralization takes place. (NaNO3 neutral salt) At…

Q: What is the pH of a saturated solution of magnesium hydroxide (the active ingredient in the antacid…

A: Milk of magnesia which is a saturated solution of magnesium hydroxide has a pH of about 10.0 (basic…

Q: If 4.5 moles of nitric acid falls into 8000 L of pure water, what will be the change of the pH of…

A: concentration = mole / litre concentration = 4.5/8000L [ H+]= 0.5625 × 10-3…

Q: A buffer solution contains 0.386 M KHCO3 and 0.312 M Na,CO3. If 0.0356 moles of hydrobromic acid are…

Q: What volume of 0.500 M HNO2 should be added to 500 mL of 0.750 M KNO2, so that the pH of the…

Q: The solubility of CaSO 4 in pure water at 0 oC is 1.09 gram(s) per liter. The value of the…

A: Let's write the dissociation equation of CaSO4 and the expression for Ksp:

Q: A 27.8 mL sample of 0.387 M trimethylamine, (CH3)3N, is titrated with 0.315 M hydroiodic acid. After…

Q: A 26.9 mL sample of 0.348 M ethylamine, C2H5NH2, is titrated with 0.391 M hydrobromic acid.…

A: The pH of a solution formed by the mixture of a weak base and its conjugate acid can be calculated…

Q: A 24.9 mL sample of 0.234 M ethylamine, C,H5NH,, is titrated with 0.315 M hydroiodic acid. After…

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, pH of a…

Q: Explain the qualitative analysis of group 2 cations

A: Dilute HCl is added to the mixture containing cations. If it dissolves completely, group 1 is…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

The mixture of 100.0 mL of 0.100 M NaOH (aq) and 100.0 mL of 0.300 M CH3COOH (aq) will result in a buffer.

(a) Explain why the resulting solution is a buffer.

(b) What is the pH of this 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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 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 solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?
A brand of window-cleaning fluid is composed of ammonia solution, water, a colouring agent, and a very small quantity of soap. It has 0.15 mol/L concentration of NH3(aq). What is the pH of this fluid?
The temperature for each solution is carried out at approximately 297 K where K w =1.00×10 −14 0.85 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution
A student added 1.78g of Ca(OH)2(9) to 0.250 L of 0.200 molL-1 HNO3(aq)- The mixture was carefully stirred until no further reaction occurred. Assuming that the total volume of the solution remains unchanged, calculate the pH of the resulting solution.
In terms of pH indicators, please fully explain what must occur in a solution to observe a colour change?
A 50.00 mL 0.750 M KOH(aq) is added to a 100.0 mL 0.500 M CH3COOH/NaCH3COO buffer. What is the expected pH of the solution?
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.
Write the expression for the solubility product constant for Pb(OH)2.
What is the significance of the Henderson-Hasselbalch equation in acid-base chemistry, and how does it relate to the pH of a solution?
A solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.
The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?