Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 49 g of NH CI dissolved in 1.00 L of 0.919 M NH,? pH (b) How many moles of acid are required to change the pH of this solution by 0.05 pH units? mol (C) Suppose 4.6 mL of 12.6 M HCI solution is added to 471 mL of the solution of Part (a). Calculate the new pH.

Q: A 20.6 mL sample of 0.377 M methylamine, CH3NH2, is titrated with 0.364 M perchloric acid. After…

A: Number of moles of   CH3NH2= M*V = 0.377 M* 20.6 mL = 7.7662 mmol Number of moles of HClO4 = M*V =…

Q: What is the pH of a buffer solution containing 0.21 M HNO2 and 0.10 M NO, ?

A: Since HNO2 is a weak monoprotic acid with pKa = 3.15  And the solution is given buffer solution with…

Q: A buffer solution is 0.467 M in HCIO and 0.321 M in NaCIO . If K, for HCIO is 3.5x10-8 , what is the…

A:

Q: How many moles of sodium hydroxide would have to be added to 150 mL of a 0.368 M hydrofluoric acid…

A: When sodium hydroxide (NaOH) reacts with hydrofluoric acid (HF), the following reaction takes place:…

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: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,) N), a weak base, and 0.20 M…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: A 2.14-g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution…

A: Sodium Hypoiodite is NaIO. It is a base and therefore, we will symbolize it by 'B' as per the…

Q: Explain the role of buffers in thecontrol of blood pH under variousconditions.

A: The role of buffers in the control of blood pH under various conditions has to be explained below.

Q: Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is…

A: Molecular weight of C6H5COOH = 122  So, 2.6 g of C6H5COOH = 2.6122mole = 0.021 mole Thus,…

Q: We have seen an introductory definition of an acid: An acid is a compound that reacts with water and…

A: Various definitions of acids and bases have been proposed from time to time. According to classical…

Q: How many liters of pure water willbe required to dissolve the same amount of solid Lead Iodate…

A: Given information:Solid lead Iodate =0.885gInitial concentration = 1.35M

Q: A buffer solution contains 0.385 M ammonium chloride and 0.444 M ammonia. If 0.0433 moles of…

A: Kb for NH3 = 1.8×10-5

Q: Which of the following statement is incorrect regarding buffer solutions: O a Maximum buffer…

A: The solution is given below -

Q: A buffer solution is 0.480 M in HCN and 0.361 M in NaCN . If K, for HCN is 4.0x10 what is the pH of…

A: This problem can be solved by using the buffer equation :…

Q: 00 grams Ca(NO,), is placed in a 1150.ml 0.015M NH, ut of solution? What is the pH of the solution?…

A:

Q: When 50mL of 0.10 M  HOAc is titrated with 25mL of 0.1O M NaOH, the pH is

A: Given, Volume of acetic acid = 50mL. Concentration of acetic acid = 0.10M. Volume of NaOH = 25mL.…

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: If 5.00g NH4Cl(s) is dissolved in 0.250M NH3, what volume of NH3 (in mL) is required to make a…

A:

Q: The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with…

A:

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…

Q: . (a) Which is the stronger base—the basic form of the indicator cresol red or         the basic…

A: Indicators are substances whose solutions change color due to changes in pH. They are usually weak…

Q: A buffer solution of 200 mL is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX.…

A: Buffer solution :- A solution which resists change in its pH value by the addition small amount of…

Q: You have at your disposal an ample quantity of a solutionof 0.100 M HCl and 400 mL of a solution of…

A: Given: Concentration of HCl = 0.100 M Volume of NaCN solution = 400 mL = 0.400 L…

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: The buffer capacity of a solution is 0.02 .How much(ml) of 1.0 M solution of sodium hydroxide NaOH)…

A: Buffer solution :- A solution which resist the change in its pH value by the addition of small…

Q: What is the pH at the equivalence point in the titration of 0.50 M KOH with 1.00 L of 0.750 M HF(aq)…

A: 1- First calculate the volume of KOH :  We will used the equation, ( M2V2)KOH = ( M1V1)HF  ( 0.50M ×…

Q: Which of the following statement is incorrect regarding buffer solutions: OBuffer solutions are…

A: Buffer solution : It is a solution formed by weak acid and it's conjugate base pr vice-versa and…

Q: Carbonic acid and sodium bicarbonate act as buffers in the blood. When a small amount of acid is…

A: We know that, our blood normal pH is 7.2 which is act as like buffer because Carbonic acid and…

Q: A buffer solution is 0.390 M in H2 CO3 and 0.348 M in КНСОЗ. If Kal for H2 CO3 is 4.2 x 10-, what is…

A: Concentration of H2CO3 = 0.390 MConcentration of KHCO3 = 0.348 MKa1 of H2CO3 = 4.2×10-7

Q: A buffer solution contains 0.341 M ammonium bromide and 0.480 M ammonia. If 0.0405 moles of…

A: On addition of an acid to the basic buffer solution, the concentration of weak base decreases…

Q: It is a common practice to prepare buffer of different pH values from a single acid. Select a single…

A:

Q: Explain how the pH of a mixture of aqueous ammonium chloride and aqueous ammonium remains constant…

A: The solution that can resist the addition of the strong acid or strong base is termed as the buffer…

Q: A 200 mL buffer solution is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX. Since…

A: A mixture of weak acid (HX)  and its salt (NaX) with strong base acts as acidic buffer solution. For…

Q: [References] Use the References to access important values if needed for this question. A buffer…

A: Henderson-Hasselbalch equation: pH of the buffer solution is calculated by using below equation. It…

Q: 100ml of solution contains 0.4 gm caustic soda. in dissolved state. If 50ml of this solution is…

A: Caustic soda is NaOH with molar mass = 40 g/mol Hence moles of NaOH taken X molar mass of NaOH =…

Q: What volume of 0.200 M HCl must be added to500.0 mL of 0.300 M sodium mandelate to producea buffer…

A: The no. of moles of solute to the volume of solution in litres is known as molarity.

Q: A weak acid indicator HIn is blue while its conjugate base In- is green. Ka,In for the indicator is…

A: Solution- pH -is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being…

Q: A buffer solution contains 0.268 M ammonium chloride and 0.311 M ammonia. If 0.0169 moles of…

A: Given -> Molarity of NH4Cl = 0.268 M Molarity of NH3 = 0.311M Moles of HI = 0.0169 mole Volume of…

Q: How many grams of Na2HPO4*2H2O must be added to 400 mL of 0.200 M H3PO4 to give a buffer of pH 7.30?

A: This question can be easily solved on the basis of the Handerson Hasselbach Equation which explains…

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: HCl is used to recover oil in oil wells by dissolving rocks, so the oil will flow more easily. In…

A: Given: Percent by mass i.e. %(m/m) of HCl = 10 % And density of solution = 1.073 g/mL.

Q: Caleulate the pH of the following two buffer solu- tions: (a) 2.0M CH;COONA/2.0 M CH3COOH, (b) 0.20…

A: a) Given: Concentration of CH3COONa = 2.0 M Concentration of CH3COOH = 2.0 M

Q: A certain organic base of the general formula ROH serves as an indicator in a neutralization…

A:

Q: A buffer solution is 0.302 M in Н2СОЗ and 0.305 M in NaHCOз. If Kal for На СОз is 4.2 × 10¬', what…

A: Henderson - Hasselbalch equation is:pH = pKa + log [Salt]/[Acid]                           . . . (1)…

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.