a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to K+CH3CH2COO-. Ka=1.3*10-5; pKa=4.89 b) Calculate the pH of the same solution after adding 0.015M KOH c) Calculate the pH of the same solutions as in part (a) but after addition of 0.015M HBr

Q: 2. When 40.00 mL of a 0.1107 M of formic acid (HCOOH) is titrated with 18.22 mL of 0.1218 M NaOH,…

A:

Q: (Q24) What is the pH of a buffer solution that is 0.338 M in ammonia and 0.455 M in ammonium…

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Q: A Buffer Solution of CH3coofd and Na oH whose PH=5, and the Concentration of CH3 COONA (o-1M).…

A:

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: Given: Concentration of HCOOH = 0.400 M Concentration of HCOONa = 1.00 M Volume of solution = 1.00 L…

Q: A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pK a of 4.54, how many mL…

A: Given pKa of HB = 4.54 By using the equation,

Q: Caffeine (C8H10N4O2) is a neutral weak base and has a Kb= 4.1 x 10^-4. If you dissolve 85 mg in 5.00…

A: Given: Kb of Caffeine (Assuming B) is 4.1 × 10-4. Mass of B used = 85 mg = 0.085 g…

Q: a. Use the Ka values provided to chose a weak acid that can effectively buffer a solution at a pH of…

A: Given data,

Q: 20. mL of 0.25 M of HC2H3O2 is titrated with 0.40 M KOH, Calculate the pH of the solution after 15…

A:

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa?…

A: The solution of HCOOH  and  HCOONa is an acidic buffer system.The pH can be calculated using…

Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…

A: Acid and base have equal mole so they neutralise to each other and we get salt. So we will use…

Q: A student needs to prepare a buffer solution with a pH of 5.20. Assuming a pKą of 4.52, how many mL…

A: I have attached the detailed solution to the question below.

Q: What is the pH before addition of any KOH?

A: Not, as per Bartleby guidelines, we can answer only first 3 questions  Given  50.0 mL of 0.200 M…

Q: Considering the equilibrium below, which of the following is/are TRUE? CH3OH + HNO2 = CH3OH2+ +…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: A buffer solution is 0.449 M in HNO, and 0.365 M in KNO, . If K, for HNO, is 4.5×104 , what is the…

A: Introduction :  We have to calculate pH of HNO2

Q: a student is preparing a Lactic acid (HLac) buffer (Ka= 1.4 X 10-4 , PH=4.00) answer the…

A: The pH of the  buffer solution is evaluated by using Henderson-Hasselbalch equation , which is…

Q: You have 500mL of a solution 0.3 M acetic acid (Ka= 1.74x10^-5 M). The pH of the solution before and…

A: We have to calculate the pH after addition of base.

Q: |Ka for formic acid is 1.7 x 10-4 at 25°C. A buffer is made by mixing 425 mL of 0.428 M formic acid,…

A: Given: Ka of formic acid = 1.7×10-4 Concentration of formic acid (M1) = 0.428 M Concentration of…

Q: If LISA adds 50 ml of 0.060 M CH3COONa to 100 ml of 0.020 M HNO3.WHAT is the PH of resulting…

A: Since CH3COONa is a salt and HNO3 is a strong acid hence we can assume that the concentration of H+…

Q: A buffer is prepared such that [CH3COOH], = [CH3C00-lo = 0.050 M. Calculate the volume of 0.10 M…

A: Millimoles of Acetic acid = M x V   = 0.050 x 100.0  = 5.0 mmol = Millimoles of sodium acetate  Let…

Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4 and 5.4 × 10^–10,…

A:

Q: Calculating thế PH Ul a weak DUJU itiutu An analytical chemist is titrating 93.8 mL of a 0.8500M…

A: Methyl amine is a weak bade it reacts with nitric acid and forms a buffer solution. pH of a buffer…

Q: The 100. mL of buffer solution is 0.05 M in C2H3O2- and 0.10 M in HC2H3O2. What is the resulting pH…

A:

Q: What's in your Bucket (write the molecule and what type--WB, WA, SA, SB, buffer, or water) before…

A: Answer: Before the addition of NaOH, in the solution we are having C2H5NHClO4, which is the salt of…

Q: Q2.Show in detail how you would prepare 350 ml of 0.12M citrate buffer pH-5.1.(You must use the Ka…

A: Desired pH = 5.1 We chose the conjugate acid/base pair as the buffer solution whose pKa value is…

Q: What will be the pH when 50.0 ml of 2.00M carbonic acid is mixed 20.0 ml of 3.00 M sodium…

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Q: Example (52):-Calculate the volume of concentrated ammonia and the weight of ammonium chloride you…

A: So we'll calculate the volume of Concentrated NH3 and mass of NH4Cl to be added.

Q: Don’t ever mix acid with cyanide (CN) because it liberates poisonous HCN(g). But, just for fun,…

A: (a)

Q: Calculate the pH of a 0.50 M HCOOH/ 0.60 M HCOOK buffer solution, and calculate the pH when 5.00 mL…

A:

Q: t 8.40 mL of 0.100 M NaOH was added to 50.00 mL of 0.100 M acetic acid (AcOH; which resulted in the…

A:

Q: dissolve an aciad we'ak H2A in wate, the solution volume will be looml, and its pH=27 if we if you…

A: The weak acid, H2A will be dissociated in water in the following way: H2A↔2H++A= The dissociation…

Q: A 1.0m HCl solution has a volume of 20.0mL. Calculate pH of the solution that results from 3.00g of…

A: Given: Molarity of HCl solution= 1.0 M Volume of HCl= 20.0 mL= 0.020 L Mass of solid acetate= 3.00 g…

Q: When 0.20 mol of NaOH is added to 0.50 mol of weak acid HX, in a total volume of 1.00 L, the pH of…

A: This acid - base reaction between NaOH and weak acid HX form a buffer solution. So we will use…

Q: An organic monoprotic base has a pkp of 8.52. A 10.00 ml sample of 0.36 M base solution is prepared,…

A: We will draw ICE table and then calculate pH.

Q: I prepare a buffer solution by mixing 30.0mL of 0.10M HOAc and 40.0mL of 0.10m NaOAc. I divide this…

A:

Q: A solution is made by mixing 185 mL of 0.100 M formic acid (Ka = 1.7 x 10-4 ) with 190. mL of 0.100…

A: This is a case of acidic buffer solution.  Moles of HCOOH = (185*0.1)/1000 = 0.0185  Moles of HCOONa…

Q: The theoretical pK, of a weak acid is 3.54. Calculate the pK, experimental error of a solution…

A: weak acid and its salt of conjugate base with strong base forms acidic  buffer whose pH is…

Q: Calculate the pH of a solution that contains 5.18 M of weak acid HA and 1.26 M NaA. The Ka of…

A: Given :  [HA] = 5.18 M  [NaA] = 1.26 M  Ka for Weak acid (HF) = 0.00063  To calculate :  pH of…

Q: A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka =…

A: Given :-  Concentration of formic acid i.e. [HCOOH] = 0.400 M  Concentration of sodium formate i.e.…

Q: Calculate the pH of a 0.40 M solution of HF (Ka = 3.5 × 10*) before and after lg of NaF is added to…

A:

Q: Conjugate base, Molar Ratio, pOH, Salt, [H+], [OH-], pKa, and the acid

A:

Q: Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1…

A: It is given that the given quantities of solutions are existing and we have to determine which…

Q: In Trial 1 0.5 grams of KHP were dissolved in 100 mL of water and titrated with 18.56 mL of NaOH…

A: Potassium hydrogen phthalate (KHP) is a salt of weak acid that is has an acid dissociation constant…

Q: A buffer solution is 0.366 M in HF and 0.372 M in KF . If Ka for HF is 7.2×10-4 , what is the pH of…

A: In above question acidic buffer is formed so pH of solution of directly determined using formula :…

Q: (1). What will be the pH when 50.0 ml of 2.00 M carbonic acid is mixed 20.0 ml of 3.00 M sodium…

A: #1:  Given the volume of 2.00 M carbonic acid, H2CO3 = 50.0 mL * (1L/1000 mL) = 0.050 L => moles…

Q: Acetic acid (HCH3CO0 or CH3COOH) is a weak acid with a Ka = 1.80 x 105. Sodium acetate (NaCH3COO or…

A:

Q: What is [H3O+] and the pH of a solution of 0.052 M HNO2 and 0.041 M KNO2?  Hint: This is a buffer.

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: ompare statement A with B. Indicate whether Statement A is Greater than, Less than, Equal, or Cannot…

A: The correct option is as follows:

Q: Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 125 mL of a buffer hav- ing a…

A:

Q: Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M…

A: According to Henderson Hasselbalch equation  pOH = pKb + log [salt] /[base] And again  pKb = - log…

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.