What is the pH of a soln which  is 0.5 M NH3 and 0.075M NH4Cl? (kb=1.8x10-5)

Q: (b) What is the pH of 0.39 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 10-4.)

A: Methylammonium bromide dissociates into quartnary ammonium ion (CH3NH3+) and bromide ions (Br-).…

Q: What is [H*] in a 0.400 M solution of acrylic acid, CH;CHCOOH (Ka = 3.16 x 10-5)?

A:

Q: What is [H*] in a 0.240 M solution of acrylic acid, CH,CHCOOH (Ka = 3.16 x 10-5)?

A: The acid dissociation constant is the ratio of ions of the product to that of reactant when a acid…

Q: For a solution of 2.5 M H2CO3 (Ka = 4.4 x 10-7), calculate: (a) [H*] (Ь) рH (c) percent ionization

A: Given: Concentration of H2CO3 = 2.5 M Ka1 = 4.4×10-7 Ka2 = 4.8×10-11

Q: pH of the 0.025 M C65NH3Cl solution? (Ka=3.8*10^-10

A: C6H5NH3Cl is a salt of weak baseC6H5NH3Cl and strong acid HCl.pH for this type of salt is calculated…

Q: What is the pH of a system that is 0.40 M in NH3 and 0.80 M in NH4Cl? (Kb = 1.8 x10-5 )

A:

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

A: HOOC-CH2-C-      COOH|   OH|CH2-COOH ( Citric acid )  Citric acid is tribasic acid and its n.factor…

Q: What is the pH of a solution of 0.400 M CH&NH2 containing 0.310 M CH:NH:l? (Kb of CH:NH2 is 4.4 × 10…

A: • According to Bartleby guidelines, I need to solve only first question in case of multiple…

Q: What is the pH of a 0.860 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

A: A numerical problem based on pH concept, which is to be accomplished.

Q: What is the pH of a 0.72 M solution of ammonia NH; (pK), = 4.74 at 25 C?

A:

Q: Part A Section 16.6. ss the section in What is [H3O+] in pure water at body temperature? of Kw…

A: From the ionization of water, H2O(l) + H2O(l) ----> H3O+(aq.) + OH-(aq.) [H3O+]= [OH-] Kw =…

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the pH of…

A: Record the given data, The concentration of NaCN is 0.030 M Ka of HCN is  4.9 × 10-10

Q: What are the concentrations of OH−OH− and H+H+ in a 0.00089 M0.00089M solution of Ba(OH)2Ba(OH)2 at…

A: Barium hydroxide is a base , 1 mole of Ba(OH)2 can give 2 mole of OH-  at 25oC…

Q: 5. 0.10 M KF (aq) saturated with cadmium chloride(s) [F] + [CdF'] [CdF2] + [CdF3]+ [CdF4 2] [K*]

A: We are given 0.10 M KF(aq) solution saturated with Cadmium chloride, CdCl2(s).

Q: Consider the reaction of 75.0 mL of 0.350 M C5H5N (Kb = 1.7 x 10-9) with 100.0 mL of 0.449 M HCI. a)…

A: Since your question has multiple sub parts, we will solve only first three sub parts for you. If you…

Q: Example / What volume of 0.40 M Ba(OH)2 must be added to 50 mL of 0.30 M NAOH to give a solution…

A: Molarity of Ba(OH)2=0.40 M  The volume of Ba(OH)2=y mL Molarity of NaOH= 0.30 M  Volume of NaOH=50…

Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10-4)?

A: HNO2 => H+ + NO2- Ka = [H+][NO2-]/[HNO2] Given, Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 =…

Q: 5. At 25°C, what changes in pH occur when (a) 0.0250 M HCI (b) 0.0250 M NaOH are diluted with water…

A: We have to predict the change in the pH.

Q: H¸NH, is a weak base (Kp = 5.0 × 10-4), so the salt CH, NH,NO, acts as a weak acid. What is the pH…

A: pH = -log[H+]  pOH = -log[OH-] pH + pOH = 14

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 at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s…

A: Concentration of CO2 can be calculated as follows: Where C is the concentration, KH  is the Henry’s…

Q: What is the pH of a solution containing 0.30 M NH4OH and 0.52 M NH4Cl? Kb= 1.8 x10-5

A:

Q: How would I find the pH of the two-component solution 0.115 M in NaCl and 9.56×10−2 M in KF?

A:

Q: Determine the pH of a solution that is 0.075 M (CH3),N and 0.10 M (CH3),NHCI. The value of Kb for…

A: Using Henderson hasselbalch equation:-

Q: A 0.492 M solution of a weak base has a pH of 10.59. What is the base hydrolysis constant, Ko. for…

A:

Q: 4- Prepare 0.1 M of HCI in 100ml of distilled water from 6N of HCI?

A: Molarity of a solution is the number of moles of solute present in one liter of solution. It is…

Q: Q 9 A 500.0 mL solution of 0.200 M BaCl2, the [Ba] and [CI] concentrations** ... respectively are:

A:

Q: What is the pH of a 0.47 M weak base solution (Kb = 9.55 x10-5)?

A: Given information: concentration of weak base solution is 0.47 M Kb = 9.55 x10-5

Q: What is the pH (to two decimal places) of a saturated aqueous solution of copper(II) hydroxide (at…

A: In this question we have to tell the PH of the aqueous solution of copper(II) hydroxide (at 25 °C).

Q: What is the value of Q when the solution contains 2.00×10^−3 M Ca^2+ and 3.00×10^−2 M SO4^2−?

A: The Q can be calculated by using formula Q = [Ca2+][SO4 2-]

Q: TF 68 5 pmilliiters of 16 M sulfuric acid we.re added to a solution that would fill up to be 550 ml…

A: Given, concentration of sulfuric acid sol = 16M Initial volume of sol =68.5 ml Final. Vol of sol =…

Q: What is the pH of 0.10 bicarbonate (HCO3-) solution? Kb=2.4E-8. x= ? [H3O+] = ? pH = ?

A: The solution for the first part is as follows :

Q: pH of the mixture of 0.020 M NH3 and 0.15 M NH4Cl (Kb NH3 =1.8*10^-5

A: Recall the Henderson-Hasselbalch equation to calculate pH of buffer solution       pOH=pKb +…

Q: 6. What is the pH of a 0.25 M solution of methylamine hydrochloride (CH3NH3CI)? Kb for methyl amine…

A: This ia a salt of weak base and strong acid. So apply formula for salt of weak base and strong acid.

Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5

A: Given, Molar concentration of NH4Cl = [NH4Cl] = 0.1 M Base dissociation constant of NH3 = Kb = 1.8…

Q: What is the pH of 0.025 M aqueous acetate ion? (Kb of CH3C

A: According to Ostwald’s Dilution Law and the pH (& pOH) scales, we can derive pOH =…

Q: What is [H3O+ ] (in M) in a solution of 0.063 M HCNO and 0.035 M NaCNO? (Assume Kw = 1.01 ✕ 10−14.)…

A: The concentration of H3O+ (in M) is to be determined in a solution of 0.063 M HCNO and 0.035 M…

Q: 7. If Kw = 1.0 x10-14, explain why pure water has a pH of 7. (C:2)

A:

Q: 2. Calculate the following: a) pH of a [H3O*] = 2.76 x 10-4 b) pH of a [OH¯] = 8.5 x 10-6M c) [H3O*]…

A: pH = - log [H+] [H+] = 10-PH pOH = - log [OH-] [OH-] = 10-POH pH + pOH = 14

Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?

A:

Q: what is the pH of an aqueous solution with [H3O+] = 2 x 10-14 mol L-1?

A: [H3O+] = 2 × 10-14 mol L-1  pH of the aqueous solution = ?

Q: calculate the pH of the 0.12M NH4OH solution with Kb = 1.8 × 10-⁵? How much will the pH of the…

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

Q: What is the pH of a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid…

A:

Q: If the Kp of a weak base is 7.3 x 10-6, what is the pH of a 0.28 M solution of this base? pH =

A: The value of Kb for the given weak base is = 7.3x10-6 The concentration of the base solution is =…

Q: What is the pH of a sol that is 0.15m in CH3coone and 0.20m in ch3cooh the ka of ch3cooh is 1.8x10-5

A:

Q: For a 0.0411 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What…

A:

Q: If the Kp of a weak base is 1.8 x 10-6, what is the pH of a 0.24 M solution of this base? pH =

A: Below attached file showing the details answer. All the best.

Q: What is the PH of a l.6M Soluten of Ascorble Acid, th C HG OG Kaz -5 = 8.0 x10, Ke=1.6A 10-12)

A: Given: Concentration of H2C6H6O6 = 1.6 M Ka1 of H2C6H6O6 = 8.0 × 10-5 And Ka2 of H2C6H6O6 = 1.6 ×…

Q: Why is [H3O] =[OH- ]=1.0 x 10-2 M not feasible in water? What would happen if we tried to make such…

A: Since the water has an equilibrium with H3O+ and OH- ions as per the reaction  Hence the…