Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that is 0.28  M  in  NH3  and 0.12  M  in  NH4Cl   (Kb(NH3)=1.76×10−5). a solution that is 0.17  M  in  HCHO2  and 0.27  M  in  NaCHO2   (Ka(HCHO2)=1.8×10−4)

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A: For separation of mixture, we have to choose a perticular solvent that dissolve that particular…

Q: For 280.0 mL of a buffer solution that is 0.240 M in HCHO2 and 0.315 M in KCHO2KCHO2, calculate the…

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Q: A solution is prepared that is initially 0.27M in hypochlorous acid (HCIO) and 0.34M in sodium…

A: The concentration of the hypochlorous acid The concentration of the sodium hypochlorite We have to…

Q: What is the pH of a solution

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Q: the solutions are additive and that Kp = 4.4 x 104 for methylamine.

A: The question is based on the concept of EQUILIBRIUM. we have to calculate pH of the solution…

Q: with

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

Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

A: Given: Concentration of HCl = 0.20 M Volume of HCl solution = 30.0 mL = 0.030 L…

Q: Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that is 0.28…

A: The objective of this question is to calculate the pH of a solution using the Henderson-Hasselbalch…

Q: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.16 M NH3 with 25.00 mL of 6.0 × 102…

A: pKb  = - log Kb            =  - log (1.80  * 10-5 )          = 4.745pKa = 14-pKb       = 14- 4.745…

Q: A solution is prepared at 25 °C that is initially 0.27 M in chlorous acid (HCIO2), a weak acid with…

A: Given  [HClO2] = 0.27 M [KClO2] = 0.19 M Ka of the weak acid, HClO2 = 1.1x10-2

Q: 15.0 mL of 0.450 M formic acid (HCOOH, Ka=1.8x10-4) is titrated with 0.250 M NaOH. Calculate the pH…

A: The given information is as follows: The value of Ka of the formic acid = 1.8x10-4 The concentration…

Q: Part A: A 252-mL buffer solution is 0.420 M in ammonia (NH3) and 0.303 M in ammonium chloride…

A: We would use Henderson Hasselbalch equation to calculate  initial pH.  Then , HBr which is a strong…

Q: What is the pH of the solution that results from mixing 25 mL of 2.30×102 M NH3 and 25 mL of…

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Q: calculate the pH of a solution that is made when 0.10 L of 0.24 M benzoic acid (pKa=4.19) and 3.00 g…

A: Molarity of sodium benzoate can be calculated as follows:

Q: For the following, please answer all the questions. A 45.75-mL sample of a 0.125 M solution of…

A: Hey, since you have asked multiple question, we will solve the first question for you.  If you want…

Q: A 0.100 L solution is composed of 0.500 M (CH3)2NH and 0.500 M (CH3)2NH2Cl at 25 oC. What is the pH…

A: The objective of the question is to calculate the pH of the solution after the addition of .A buffer…

Q: You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.63 M…

A: Buffer Question and finding the concentration of Salt to make a buffer of pH = 9.2

Q: An analytical chemist is titrating 150.4 mL of a 0.5000M solution of benzoic acid (HC H-CO₂) with a…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Consider the titration of HCOOH with NaOH. A 125 mL sample of 0.27 M HCOOH is titrated with 0.18 M…

A: Given the titration of HCOOH with NaOH ,as NaOH is strong base , while formic acid is not stong acid…

Q: Predict whether the following aqueous solutions have a pH less than 7, very close to or equal to 7…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: A 1.00 L solution contains 0.372 M HA (Ka = 2.93⋅10−62.93⋅10-6) and 0.741 M NaA.   What is the pH…

A: Here we are required to find the pH of the solution.

Q: Consider a buffer solution that is 0.47 M HCN and 0.47 M NaCN. (Ka(HCN) = 4.9 × 10−10) Calculate…

A: After addition of 0.20 mol of NaOH the [ HCN ] = ( 0.47 - 0.20 ) = 0.27 M And [ NaCN ] = ( 0.47 +…

Q: pose 26.5 mL of 0.19 M NaOH is added to 45.3 mL of 0.24 M HCHO2. What will be the pH of the…

A: Molarity of HCOOH= 0.24 M  Volume of HCOOH= 45.3 ml  Molarity of NaOH = 0.19 M  Volume of NaOH =…

Q: A 1.0 liter solution contains 0.25 M hydrogen fluoride (HF) and 0.38 M sodium fluoride (NaF). What…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: b An analytical chemist is titrating 136.2 mL of a 0.7100M solution of methylamine (CH3NH2) with a…

A: Given: VCH3​NH2​​=136.2mL;[CH3​NH2​]=0.7100M;VHNO3​​=97.5mL;[H+]=0.4900MpKb​=3.36;pH=???Step 1:…

Q: Calculate the pH of a solution at the equivalence point when 200.0 mL of a 0.20 M solution of Lactic…

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Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has…

A:

Q: Calculate the pH of a solution that is made when 0.10 L of  0.24 M  benzoic acid (pKa = 4.19)  and…

A: Mass of sodium benzoate = 3.00 g Molar mass of sodium benzoate = 144.11 g/mol Moles =…

Q: Calculate the pH of the following solution when the 2 reagents are mixed: 25.00mL of 0.550M HCI…

A: Answer: This question is based on the pH of buffer solution. Buffer solution is the type of solution…

Q: Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M…

A: 4-chlorobenzoic acid is a weak acid. The chemical equation for the given question may be written as:…

Q: A solution is prepared that is initially 0.087M in benzoic acid (HC H,CO,) and 0.11M in potassium…

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Q: A solution is prepared at 25 °C that is initially 0.47 Min dimethylamine ((CH,) NH), a weak base…

A: pKb = -log Kb pKb = -log (5.4 x 10-4) pKb = 3.2676 now according to hasselbalch hendersen equation…

Q: A solution contains 0.397 M HA (K₂ = 8.08. 10-6) and 0.719 M NaA. What is the pH of this solution?…

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