Kb for NH3 is 1.8 × 10-5. What is the pH of a 0.45 M aqueous solution of NH4Cl at 25.0 °C? Show

Q: Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3…

A: The pH of a solution can be calculated as follows: pH= 14-pOH where pOH = -logOH- To calculate…

Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…

A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given :- concentration of methylamine solution  = 0.0730 M  Kb for methylamine = 4.4 × 10-4  To…

Q: What is the pH of a 0.350 M triethylamine, (C2H5)3N, solution?             Kb for triethylamine is…

A: Given, 0.350 M triethylamine  Kb for triethylamine is 5.3 *10-4

Q: 28. What is the pH of a 0.62 M NH,NO, solution at 25°C? [Kb for NH; is 1.76 × 10°] А. 2.48 В. 4.73…

A: Welcome to bartleby !  We have to calculate pH

Q: A 1.00 L solution contains propanoic acid (C3 H5 O2 H) with a concentration of 0.350 mol/L, and…

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Q: Calculate the OH- for a 0.300 M solution of pyridine, Kb = 1.7 x 10^-9

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Q: What is the pH of a 0.0600 M solution of nitrous acid at 25 C?

A: Since nitrous acid is a weak acid with acid dissociation constant = 5.6 X 10-4  The dissociation…

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: What is the pH of a 3.6×10-2 M solution of KOH at 25 °C?

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Q: Dimethylamine, (CH3)2NH, a key intermediate in detergent manufacture, has a Kb of 5.9 x 10-4. What…

A: Ionic equilibrium is the equilibrium which is established between the unionized molecules and the…

Q: what is the ph of a 0.85 M solution of pyridine (C5H5N, Kb = 1.70 x 10 ^-9)

A: Pyridine is a weak base. pOH of a weak base. pOH = -log [OH-] pH = 14 - pOH For a weak base like…

Q: Show complete calculations for the pH of a 0.105M solution of ammonium chloride. The Kb for ammonia…

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Q: What is the pH of a 0.1966 M HCOOK? Ka for HCOOH is 1.74e-4.

A:

Q: What is the PH of a 0.01 M solution of salt NaA, where A- is the anion of an acid whose ionization…

A: Given that,  Concentration of salt NaA, = 0.01 M Ionisation constant Ka   = 10-6 pH of the given…

Q: The Ka of acetic acid is 1.80 x 10-5.  A. What is the pH of a 0.0010 M solution of acetic acid? B.…

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Q: What is the pH of an aqueous solution that is initially prepared as  0.35 M  NH4Br ?    Note:  Kb…

A: NH4Br is a salt formed from a strong acid HBr and a weak acid NH3. Therefore the salt is acidic.The…

Q: What is the pH of a 3.9×10-2 M solution of KOH at 25 °C?

A: KOH ionizes in aqueous solution as,                          KOH (aq)       -----> K+ (aq)   +…

Q: Calculate the pH of 0.564 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5)

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Q: 13.3) Determine [OH–], pOH and pH of a 0.18 M  aqueous solution of LiC3H5O3 (K b = 7.1×10-11).

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Q: What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid…

A: Given that ,  Initial concentration of valeric acid = 0.32 M  Dissociation constant , Ka = 1.44×10-5…

Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: Pyridine has Kb = 1.7 x 10-9. What is the pH of a 0.10 M pyridine solution?

A: Pyridine is a weak base. For a weak base solution: [OH-] = (Kb x C)1/2 pOH = -log[OH-] pH + pOH = 14

Q: 6- Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution…

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Q: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…

A: Given,  for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…

Q: The pH of a solution at 25°C in which [OH]= 2.0 x 10 is: 1 9.52 4.76 4.69 3.30 9.30

A: In this question, we want to determine the pH of the Solution.  You can see details Solution below…

Q: What is the pH of a 0.0100 M  solution of analine (C6H5NH2) , a weak base.     Kb= 4.0 x10-10

A: The chemical equation for aniline can be written as: This equation shows that aniline is a base,…

Q: Kb for ammonia (NH3) is 1.76 x 10-5     What is Ka for ammonium, its conjugate acid. (NH4+)

A:

Q: Hydroxylamine, HONH₂, readily forms salts such as hydroxylamine hydrochloride which are used as…

A: According to the question we have, The concentration of the hydroxylamine (HONH2) is given by (c) =…

Q: 5c. What is the pH of a solution which is 0.0400 M in potassium isocyanate (K* CNO") and 0.0300 M in…

A: Given, [K+CNO-] = 0.0400 M            [HOCN] = 0.0300 M As , K+CNO- is a salt it remains as…

Q: Calculate the pH of a 0.05 M solution of hydrofluoric acid. The Ka of hydrofluoric acid is 6.6x10^-4

A: Given data, Molarity of HF=0.05MKa of HF=6.6×10-4 pH of a solution is given by -log[H+]

Q: A solution is prepared at 25 °C that is initially 0.16 M in ammonia (NH3), a weak base with K₂ = 1.8…

A:

Q: The Ka of hypochlorous acid (HClO) is 3.00 × 10^-8. What is the pH at 25.0 °C of an aqueous solution…

A: Given- Ka of hypochlorous acid =3.00×10-8 Concentration of hypochlorous acid =0.0200M

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: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4.  What is the pH of a 0.290 M  solution of methylamine?

A:

Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4  The dissociation…

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: given  HClO Ka=4.0 x 10-8  concentration of  NaClO IS 0.027  PH =?

Q: Calculate the molar concentration of OH- in a 0.075 M solutionof ethylamine (C2H5NH2; Kb = 6.4 x…

A: The reaction taking place is  => C2H5NH2 (aq) + H2O (l) -----> C2H5NH3+ (aq) + OH- (aq)  Hence…

Q: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

A:

Q: For H2CO3, Ka1= 4.3 x 10^-7, Ka2= 4.7 x 10^-11. What is the pH of a 0.28 M solution of carbonic…

A: H2CO3 is a weak acid.  pH = 0.5pKa - 0.5logC ....(1) Here, pKa1 = -logKa1 = -log(4.3*10^-7) = 6.37…

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

A:

Q: The acid dissociation constant for acetic acid (HC2H3O2, commonly abbreviated HAc) is 1.8 x 10-5.…

A: Given, Acid dissociation constant, Ka = 1.8*10-5. Molarity of acetic acid solution = 0.10M. The…

Q: What is the pH of a 0.0680 M solution of hydrocyanic acid, HCN (Ка %3D 4.9 х 10-10)?

A:

Q: Calculate the molar concentration of OH− ions in a 0.077 M solution of ethylamine (C2H5NH2;…

A: Given, Concentration of the ethylamine solution (C) = 0.077 M Kb for ethylamine (C2H5NH2) = 6.4x10-4…

Q: A.) What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic…

A:

Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: The pH of a solution at 25°C in which [OH-] = 3.7 x 10-5 M is: 4.43 3.70 4.78 8.6 D 9.57

A: Given OH- = 3.7 x 10-5

Q: How many milligrams of CH3COOH (fw 60) should be added to 250 mL of water to get pH 3. K. = 1 x 10-5

A: CH3COOH is weak acid in aqueous solution. It will dissociate in solution as below-

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: pH = 7 +12 (pka + log c)