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

Q: What is Kb for the conjugate base of HBRO (Ka = 2.5 x 10°)?

A: HBrO Ka = 2.5 * 10-9

Q: The Ksp of aluminum hydroxide, Al(OH)3, is 2 × 10−31. What pH is required to limit the Al3+…

A: Al(OH)3 (s) ------> Al3+ (aq) + 3 OH- (aq) The Ksp of the reaction is given by  Ksp = [Al3+] X…

Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is 1.8 x 10-5

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Q: Calculate the pH of 2.50M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)

A: The ICE table are utilized to figure out the hydrogen ion's concentration. With the help of hydrogen…

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: 6- Calculate the pH of a 8.0 x 10 ´M aqueous solution of hydrobromic acid (HBr). Round your answer…

A: The pH is to be calculated

Q: When [H+] = 4.0 x 10^-9 M in water at 25 degrees Celsius. What is the pH?

A: Given : [H+ ] = 4.0 X 10-9 M

Q: What is the pH of a 0.21 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25 degrees C?

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Q: What is the pH of a peach with a [OH¯]=3.2x10-11 М ОН"?

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

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

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

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Q: Hydroxylamine (NH2)H) is a weak base with a Kb=6.6x10^-9.  What is the pH of a 0.36 M solution of…

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Q: The pH of a 0.045 M Ca(OH)2 solution is: +1.3467 O +12.954 O +12.653 O -1.3467

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Q: What is the pH of a 0.144 M solution of ammonia (Kb 1.8 x 10-5)?

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Q: When the pH is 7, there is no H30* or OH in solution.

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

Q: Determine the pH of a 2.79 M solution of acetic acid (CH3COOH, ka=1.8x10-5)

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Q: What is the pH of a 0.150 M solution of acetic acid (pKa=4.75) at 25 degree celsius?

A: Given, the concentration of acetic acid =0.150 Mand pKa of acetic acid =4.75 at 25 °Cwe are asked to…

Q: When [H+]=4.0 x 10(-9) M in water at 25 C, what is the pH

A: Given that Concentration of H+ = 4.0×10-9 M

Q: What the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 10*)?

A: A numerical problem based on pH of the weak base, which is to be accomplished.

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: The pH of a 0.02 M NgOH solution at 25 °C is: O 12.8 O 13.7 O 1 1.5 O 12.3 O 13.1

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Q: What is the pH of 0.0005 M HNO3?

A: The given data is as follows: The concentration of HNO3 = 0.0005 M As we know that HNO3 is a strong…

Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

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

Q: Calculate the pH of a 1.50 M (CH»),NHB solution (aq., 25 °C). 3) Kb (CH3)N - 6.31 x 105

A: (CH3)3NHBr is a salt of weak base and a strong acid formed by the reaction of  trimethyl amine…

Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: What is the pH of a solution prepared by adding 60.4 g ethylammonium chloride (C2H5NH3CI, 81.55…

A: As C2H5NH3Cl is salt of weak base and strong acid while C2H5NH2 is weak base so the resultant…

Q: Calculate the pH of a 2.0 x 10–3 M solution of pyridine (C5H5N). Kb = 1.7 x 10–9

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

A:

Q: What is the pH of a 0.21 M solution of methylamine

A: Given :-  Initial concentration of CH3NH2 solution = 0.21M  Kb = 4.4 × 10-4  To calculate :-  pH of…

Q: (a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-. (b) Give…

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Q: What is the pH of 0.80 M methylamine (CH3NH2). Kb = 4.4x10-4.

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Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

A: pH of solution is calculated using relation pH + pOH = 14

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: What is the pH of a 3.0 x 10 M solution of CoHsNH2 (Kb= 4.3 x 1010? What is the percent error in…

A: As PhNH2 is an weak base,it can be calculated using a formula.

Q: What is the pH of a 0.02M ammonia solution if its Kb value is 1.8*10^.5? H.O + NH, 2 OH + NH,. 3.2 O…

A: The value of Kb for the given weak base is = 1.8×10-5 The concentration of the base solution is =…

Q: Which of these aqueous solutions is expected to have the highest pH at 25 °C? 0 1.0 М Са(ОН)2 0 1.50…

A: pH of Acid is below 7 and pH of base is above 7.

Q: Write the formula of the conjugate acid of the Brønsted-Lowry base, C₄H₃N₂O₃⁻ ?

A: If we add H+ in base then it will convert into conjugate acid   C₄H₃N₂O₃⁻ +H+= C4H4N2O3

Q: Calculate the [OH-], [H3O+], pOH and pH of a 0.075 M NH3 Ka NH4+ = 5.70 x 10-10

A:

Q: What is the pH of a 0.0570 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 1010)? %3D

A: HCN is a weak acid. Hence it will dissociate partially as per the reaction HCN -----> H+ + CN-

Q: What is the pH of 5.04 x 10-3 M HI? Is it acidic, basic, or neutral?

A: HI is a strongest acid it dissociates completely .

Q: The value pKw is 11.05 at 78 °C. What is the pH of a neutral solution at the same temperature? Enter…

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Q: The Kb of pyridine, C5H5N, is 1.7 x 10−9.  Calculate the pH of a 0.124 M solution of pyridinium…

A: Given: The Kb of pyridine (C5H5N) = 1.7 x 10−9  The molarity of the solution of pyridinium bromide…

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (CH3O;)? CsH2Or(aq) +…

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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 a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: The Kb for aniline (C6H5NH2) is 4.3 x 10-10. What is the pH of a 0.15 M solution of aniline?

A: From the ICE table, we have

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

A:

Q: ph of 0.10 M NaNO2 (Ka of HNO2 is 4.5 x 10-4 ?

A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4

Q: Consider the following acid-base pairs: H2CO/ HCO K 42 x 107 H;PO4/HPO K, = 6.2 x 10 NH/ NH3 K, =…

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