What is the pH of 0.133 M trimethylammonium iodide, (CH3)3NHI? At 25°C, the Kb of trimethylamine, (CH3)3N, is 6.3 x 105. Enter your answer in decimal format with two decimal places (value + 0.02).

Q: In the laboratory, a general chemistry student measured the pH of a 0.548 M aqueous solution of…

A:

Q: The pH of a 1.4M solution of acetic acid (HCH,CO,) is measured to be 2.30. Calculate the acid…

A: Given- pH=2.30 Concentration of acetic acid= 1.4M

Q: Look up the appropriate Ka1 and Ka2 values for oxalic acid andascorbic acid, and repeat these…

A: The first and second dissociation constants of oxalic acid have been mentioned as follows-

Q: Calculate the pH of a 0.0500M solution of phenylacetic acid, C6H5CH2COOH and  0.0200M with its salt,…

A: Given,  The pH of a 0.0500M solution of phenylacetic acid, (C6H5CH2COOH) and  0.0200M of its salt,…

Q: 11. The ionization constant, Kw, of water at 60 °C is 1.00 x 10-13. What is the pH of pure water at…

A: Given Kw = 1.00 x 10-13

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: What is the concentration of (OH] in this solution? Calculate your answer in M, then provide the…

A: Given data :-

Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 x 10. Calculate the pH of a 1.3…

A: Reaction: C4H4N3O3NH2 + H2O ⇌ C4H4N3O3NH3+ + OH-    Kb of allantoin = 9.12×10-6  Concentration = 1.3…

Q: n the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of…

A: Here we have:Concentration of diethyl amine = 0.354 MKb= 6.9 × 10-4

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

A:

Q: What is the pH of a solution prepared by combining 0.696 mol of a weak acid (Ka = 5.5 x 10-5) with…

A: we need to calculate pH of the solution

Q: What is the pH of a 0.220 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Aniline is a weak base.  C6H5NH2+H2O⇔C6H5NH3++OH-      1                                  0…

Q: In the laboratory, a general chemistry student measured the pH of a 0.458 M aqueous solution of…

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

Q: calculate the pH and degree of dissociation

A:

Q: What is the ionization constant at 25 °C for the weak acid (CH3)2 NH2 +, the conjugate acid of the…

A: The weak base given is (CH3)2NH. Conjugate acid of any weak base is produced when the base accepts a…

Q: the laboratory, a general chemistry student measured the pH of a 0.428 M aqueous solution of…

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: Abbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2…

A: a.

Q: What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine. CH3NH2. with 25.00…

A: Given : Concentration of methamine i.e CH3NH2 = 0.10 M Volume of CH3NH2 solution = 25.00 mL = 0.025…

Q: What is the pH of a 0.290 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Find PH using ICE table and some farmula

Q: The pH of a 0.052M solution of acrylic acid (HC,H,CO,) is measured to be 2.77. Calculate the acid…

A: GivenpH = 2.77pH = -logH+2.77 = -log H+H+ = 0.00169 M[H+] = 1.7 * 10-3 M

Q: What is the pH of a 0.710 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A:

Q: An aspirin tablet contains 250 mg of acetylsalicylic acid, C9H8O3 (Ka = 6.4x10-4).  If you take the…

A: Answer :- pH = 2.30  pH of mixture of 250 mg acetylsalicylic acid, C9H8O4 in 35.0 mL water is 2.30…

Q: What is the pH of a 0.050 M triethylamine, (C2HS)3N, solution? Kb for triethylamine is 5.3 x 10-4

A: We should know that the amine us a basic Compound that will dissociate in solution to give basic…

Q: Calculate the pH of a 0.0076 M solution of acetic acid, CH3COOH. The Ka of acetiç acid = 1.8 x 10-5.…

A: Kaa of acetic acid = 1.8× 10- 5  initial concentration of acetic acid = 0.0076 M

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

A: pH of a solution is used to define acidity or basicity of the solution. At room temperature, pH of…

Q: used as preservatives in vinegar, soy sauce, etc. The pH of a 0.10 M aqueous solution of sodium…

A: Sodium benzoate is salt of weak acid-strong base type salt pH = 1/2(14 + pKa + log([C]) 8.60 =…

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: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 x 10 °. Calculate the pH of a…

A: Given Initial Concentration = 0.47 M Kb = 9.12 × 10-6

Q: Aniline, C6H5NH2, is a weak base with K, = 3.8 x 10-10. What is the pH of 0.750 M anilinium chloride…

A: Anilinium chloride is a salt made from strong acid HCl and weak base aniline.  So, solution of…

Q: The initial molar concentration of formic acid (HCOOH) is 1.7 M. What  is the pH of the solution, if…

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

Q: In the laboratory, a general chemistry student measured the pH of a 0.400 M aqueous solution of…

A: To find Kb for base, first write reaction of base with water and according to that, find [OH-] or…

Q: In the laboratory, a general chemistry student measured the pH of a 0.552 M aqueous solution of…

A:

Q: Calculate the pH of a 0.0607 M solution of trimethylamine. The Kp of trimethylamine, (CH3)3N, is…

A: Kb  of trimethylamine = 6.4× 10-5  Initial concentration of trimethylamine = 0.0607 M

Q: Calculate the pH of a 0.094 M solution of formic acid, H2CO2. The Ka of formic acid 4 x 10-4 Submit…

A: In case of weak acids , the H+ ion concentration is given by the following formula  [H+] = (Ka×C)1/2…

Q: What is the ionization constant at 25 °C for the weak acid (CH3)2NH2+,the conjugate acid of the weak…

A: Formula for relationship between ka and kb is  ka*kb= 10-14 Ka= 10-14/kb Ka= 10-14/5.9x10-4 Ka=…

Q: In the laboratory, a general chemistry student measured the pH of a 0.522 M aqueous solution of…

A: pH is defined as negative logarithm of hydrogen ions.

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: What is the pH of a solution of 50.00 mL of 0.07500 M hydroxyacetic acid, Ka = 1.48 x 10^-4, after…

A: Concentration of solution = 0.07500 M Acidic constant of solution = 1.48 × 10-4       Volume of…

Q: Trimethylamine, (CH3)3NH2, is a gas with a fishy, ammonialike odor. A 0.25 M aqueous solution of…

A: Since you have posted multiple questions, we are entitled to answer the first only. NOTE : The…

Q: A1.12 M solution of a weak acid has a pH of 2.73. What is the pKa of the acid? Report your answer to…

A:

Q: Methyl Amine (CH3NH2) is a weak base with a Kb of 4.38 x 10-4. What would be the pH of a solution of…

A: The above salt is a mixture of weak base and strong acid. When it dissolves in water it forms an…

Q: Calculate the pH that results when 2.35 mL of a 0.0125 M aqueous solution of KOH is added to 23.50…

A: On addition of KOH, it reacts with the conjugate acid CH3NH2 and hence increases the concentration…

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: The Kb of a weak base, Z, is 3.75 x 10−12.  What is the Ka for its conjugate acid, HZ+?

A:

Q: What is the pH of 0.0850 M  Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)?  Express your answer to two decimal…

A: Given concentration of Fe(NO3)3 is 0.0850 M

Q: What is the pH of 0.541 M dimethylammonium iodide, (CH3)2NH21? At 25°C, the Kb of (CH3)2NH is 5.9 x…

A: Dimethylammonium iodide is a salt of a strong acid, HI, and weak base, (CH3)2NH. So, in this case,…

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

A:

Q: The acid dissociation constant K of alloxanic acid (HC,H,N,05) is 2.24 x 10 a. Calculate the pH of a…

A: [HA] = 2.8 M ( concentration of alloxanic acid ) Ka = 2.24 × 10-7 pH =?

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.