What is the pH when 10 mL of 0.144 M HC2H3O2 ( Ka= 1.80*10^-5) is titration with 55 mL of 0.183 N KOH?

Q: What is the pH of a solution prepared by mixing 25.0 mL of 0.180 M HC,H30, with 40.0 mL of 0.250 M…

A: pH of the solution = 13.71

Q: 100.0mL of a 0.050M HNO2 solution is titrated with a 0.10M NaOH solution. How many mL of NaOH would…

A: Let the volume of NaOH = V mL pH = 3.39 Molarity of HNO2 = 0.050M Molarity of NaOH = 0.10 M

Q: a 500 ml solution containing 0.01 m of acetic acid (ch3cooh) has a ph value of 3.38. how many…

A: For a weak acid such as CH3COOH, the concentration of H+ is given as, H+=Ka×C1/2 When NaOH is added…

Q: What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 20.00 mL of 0.10 M…

A: Given, NH3= 20mL of 0.1M Kb= 1.8× 10-5 NH3 = Weak base NH4Cl = Salt This is a buffer solution…

Q: What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95…

A: We will calculate the number of moles of each reactant and then draw ICE table to calculate pH of…

Q: What is the pH of the medium and Ka of this acid when 10 percent of the weak acid, 0.01 M HX acid,…

A: The dissociation reaction of weak acid HX is  HX ------> H+ + X-

Q: 12. Pyridine, CSH§N is a weak base with Kb = 1.7 x 10". How many moles of pyridinium chloride,…

A: Henderson-Hasselbalch equation for bases: pOH = pKb + log ([B+ ]/[BOH]) where "pKb" is the base's…

Q: A few mL of 0.800M HCl are added to 20mL of 0.800. NaC2H3O2. Will the initial pH of the 0.800M…

A: pH is used to determine the concentration of hydronium ion. pH for acid is less than 7. pH for base…

Q: Given 0.10 M NaCn with a Ka value of HCN at 6.2 x 10-10 What is its pH?

A:

Q: In the titration of 25 ml of O.O50 M HCl with 0.050 M NaOH, what is the pH a. before any NaOH is…

A: Since you have posted questions with multiple subparts, we will solve only the first three subparts…

Q: What is the pH of a 0.220 M solution of sodium cyanide (NaCN)? Ka for HCN is 4.9 x 10-9.

A: NaCN has one less hydrogen and corresponds to a conjugate base (a weak base). The credentials…

Q: What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate base…

A: The solution is given below -

Q: 5.0 mL of 0.100 M NAOH is added to 50.0 mL of 0.100 M hypochlorous acid (HCIO). If the K, of…

A:

Q: In a titration of 13.5 mL of a 0.425 M solution of a diprotic acid H2C4H&O6 (tartaric acid) with…

A: Volume of tartaric acid = 13.5 ml  Molarity of tartaric acid = 0.425 M  Molarity of LiOH = 0.155 M…

Q: What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A:

Q: 1. Calculate the pH of a 200.0-mL solution containing 0.050 M benzoic acid (C6H5COOH) and 0.025 M…

A: pH = pKa + log[C6H5COO-]/[C6H5COOH]

Q: 2) What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate…

A:

Q: In a titration of 26.5 mL of a 0.425 M solution of a diprotic acid H2C4H4O6 (tartaric acid) with…

A: Moles of base =  2 × moles of acid

Q: You have a 0.189 M solution of propanoic acid.  You add enough sodium propanoateto make the solution…

A:

Q: What is the pH of a solution that is 0.75 M HF and 0.15 M NaF?   The Ka of HF is 6.6 x 10-4

A: Given: Concentration of HF [HF]= 0.75 M Concentration of NaF [NaF]= 0.15 M Ka of HF is 6.6 x 10-4 To…

Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…

Q: If a buffer solution is 0.240 M in a weak acid (Ka = 8.1 × 10-5) and 0.430 M in its conjugate base,…

A: Given,Concentration of salt is given as a 0.430 MConcentration of acid is given as a 0.240 M

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

A:

Q: pH

A:

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 50.00 mL of 0.100 M…

A: Since the moles of acetic acid = molarity of acetic acid X volume in L = 0.1 X 30/1000 = 0.003 And…

Q: If

A: Given: 50 mL of 2.00HCN(Ka=6.210×10-10) is diluted to 1.00 L. To find: pH of the solution.

Q: When titrating a strong monoprotic  acid  with NAOH at 25C the :

A: We have to predict the correct option for titration of monoprotic acid with NaOH.

Q: At what volume of  NaOH titrant (in mL) is the equivalence point reached when 10.0 mL of 1.00M HCl…

A: An unknown concentration of one solution is determined from the known concentration of other…

Q: What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to…

A:

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 mL of 0.10 M…

A: Weak acid are those which does not dissociate completely in aqueous solution. Here all CH3COOH are…

Q: In a titration of 56.0 mL of a 0.400 M solution of a diprotic acid H,C,Oa 2H,O (oxalic acid…

A:

Q: The weak acid HXO2 has a dissociation constant of Ka = 6.50 x 10-10. A lab worker prepares of 0.600…

A: We will calculate pH

Q: In the titration of 25 ml of O.O50 M HCl with 0.050 M NaOH, what is the pH a. before any NaOH is…

A: pH: It can be defined by saying the concentration of hydronium ion in any solution. Depending upon…

Q: t is the pH when 50 ml 0.1 M NaOH is added to 50 ml 0.1 M HA? (Ka= 104)

A: This can be solved by ph calculation of weak acid and strong base .  Answer is not matching with…

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: Calculate the volume at which the pH= pKa if 30.00mL of weak acid with a concentration of 0.09885M…

A: Concentration of weak acid (M1) = 0.09885 M Volume of weak acid (V1) = 30.00 mL Concentration of…

Q: how you determine the pH when 15 ml of 0.100 M HCI is ado 080 M NH3 (K, = 1.6 x 10-6)

A: Given,  Kb = 1.6×10-6 pKb = -log(Kb) = -log(1.6×10-6) = 5.82 Molarity of HCl = 0.100 M Volume of HCl…

Q: What is the pH of a solution when 82.5 mL of a 0.1M HCN solution (ka = 6.2 x 10 -10) is titrated…

A: pH of a solution is the negative logarithm of the H+ ion concentration. In acid-base titrations, one…

Q: Q. 4 A buffer is prepared by adding 115 mL of 0.30M NH3 to 145 mL of 0.15M NH,NO3. What is the pH of…

A: We will solve this problem using the Henderson equation

Q: If a buffer solution is 0.200 M in a weak base (K = 1.9 x 10-5) and 0.420 M in its conjugate acid,…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5. What will be the pH of a 0.10 M…

A: Given, The ionization constant of acetic acid HC2H3O2 is 1.8 x 10-5 0.10 M HC2H3O2 and 0.10 M in…

Q: A 30.00 mL sample of 0.15 M HNO3 is titrated with 0.20 M KOH. Calculate the pH when 25.00 mL of…

A:

Q: A 20.00 mL of 0.100 M diprotic weak acid H2A is titrated with 0.200 M NaOH. The volume of the NaOH…

A:

Q: a) Calculate the pH of a buffer solution made by combining 3.S09g of NaOAc •3H,0 (Sodium Acstehe

A: Given: Mass of NaOAc.3H2O = 3.509 g Volume of HOAc =8.8 mL Volume of water added= 55.6 mL

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

A:

Q: In the titration of 100.0 mL of 0.050 M HCl solution, what will be the pH after adding 30.0 of a…

A: Molarity = number of moles/volume (L)  So, moles = molarity × volume (L)  pH = -log[H+]

Q: If a buffer solution is 0.260 M in a weak acid (Ka=2.4 •10^-5) and 0.560M in its conjugate base,…

A: Given : Concentration of weak acid = 0.260 M Concentration of its conjugate base salt = 0.560 M And…

Q: What is the pH of a solution made by mixing 10.00ml of 0.10M acetic acid with 10.00 ml of 0.10M KOH?…

A:

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.