What is the pH of 0.541 M dimethylammonium iodide, (CH3)2NH21? At 25°C, the Kb of (CH3)2NH is 5.9 x 10-4. Enter your answer in decimal format with two decimal places (value ± 0.02).

Q: What is the pH of 0.125 M  Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)?  Express your answer to two decimal…

A: Given that 0.125 M Fe(NO3)3 is present. Fe+3 has a Ka value of 3.00×10-3. The equation used to find…

Q: Calculate the pH at 25 °C of a 0.80 M solution of potassium butanoate (KC, H,CO,). Note that…

A: Given,  [KC3H7CO2] = C = 0.80 M  pKa value of HC3H7CO2 = 4.82  Calculate the pH = ?

Q: Calculate the pH of a 0.86 M solution of a weak base CH3NH2 (Kb = 1.8 x 10-5) Write a chemical…

A:

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 )

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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: Would you expect a solution of ammonium chloride (NH4Cl) to be acidic or basic when added to water?…

A: Introduction- For the salts of strong acids and strong bases, the pH of salt will be neutral that is…

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: Aniline C,H5NH2 (K, = 3.8 x10-10) is a weak base. Calculate the pH and pOH of a 50.0 mL solution of…

A: Hydrolysis of weak base : Hydrolysis means dissociation in presence of water. When a weak base like…

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

A: pH is used to determine the concentration of hydronium ion.

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: What is the pH of a 0.10 M H2C2O4 solution that has the stepwise dissociation constants Ka1 = 5.9 ×…

A:

Q: The base protonation constånt K, of morpholine (C,H,ONH) is 2.14 x 10 . Calculate the pH of a 0.86 M…

A: Equilibrium constant is the ratio of  product of concentration of products raised to their…

Q: A general chemistry student measured the pH of a 0.12 M aqueous solution of an unknown weak acid HA…

A: The question is based on the concept of equilibrium. we have to calculate PKa of a weak acid whose…

Q: I have ammonia (.105M) dissociating in water.  What is the pH?  Kb=1.8E-05

A:

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: 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: What is the calculated pH of the initial 0.100M Acetic Acid solution?  Ka = 1.8 x 10-5 .  Give your…

A: The dissociation reaction of acetic acid is given below: CH3COOH(aq) + H2O(aq) ⇌ CH3COO-(aq) +…

Q: The Kb of aminoethanol, HOCH2CH2NH2 is 3.1 x 10-5  Write ionization equation of the aminoethanol in…

A: The species which gets formed after accepting a proton in specified solution is "conjugate acid"…

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

A:

Q: Find the ph and the percent hydrolysis of a 0.0335 M solution of pyridine hydrochloride (the salt of…

A: Given : Concentration = 0.0335M

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: iii. Given that at a particular temperature the ionic product of water is 1.00 x 10-14 moldm“,…

A: iii) Given: Concentration of sodium hydroxide i.e. NaOH = 0.05 M

Q: What is the pH of 0.133 M trimethylammonium iodide, (CH3)3NHI? At 25°C, the Kb of trimethylamine,…

A: Given Concentration of triethylammonium iodide is 0.133M Kb for triethylamine is 6.3 X10-5 We have…

Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…

A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 oC.  At the same temperature, Ka for HBrO2…

A: Answer: Conjugate acid of weak base and conjugate base of weak acid gets hydrolyzed on adding in…

Q: When 2.0 x 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH…

A: Nicotine is a weak monoprotic acid so it dissociated in less amount. So we can denotes it by HA .

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: 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: 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: Cyanic acid (HCNO) has Ka = 2.0 x 10-4 What is the conjugate base and its Kb value?

A: A conjugate acid is formed by the removal of -OH  from a base and a conjugate base is formed by the…

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: What is the pH of 0.31 M diethylammonium chloride, (C2H5)2NH2Cl.  The Kb of diethylamine, (C2H5)2NH,…

A: The pH of the 0.31M diethylammonium chloride is given below

Q: Ascorbic acid (vitamin C, C6H8O6) is a cliprotic acid (Ka1= 6.8 x 10-5 and Ka2 = 2.7 x 10-12). What…

A:

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: 2. Calculate the pH of a solution containing 0.75 M lactic acid, HC3H5O3, (Keq= 1.4 x 104) and 0.25M…

A: The solution contains a mixture of 0.75 M lactic acid and 0.25 M sodium lactate.

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 0.278 M diethylammonium iodide, (C2H5)2NH2I.  The Kb of diethylamine, (C2H5)2NH,…

A:

Q: Given,  Molarity of glycine hydrochloride (say HA) = 0.1 M  Volume of glycine hydrochloride = 20…

A:

Q: The acid dissociation constants for sulfurous acid, H2SO3, are K, = 1.7x102 and K," = 6.4x108. What…

A:

Q: Calculate the pH of a 0.500 M solution of the amino acid, asparagine, that was prepared from the…

A: Asparagine is a non-essential amino acid which is used in the biosynthesis of proteins. It has the…

Q: Calculate the pKa of the weak acid HA, given that a solution that is 0.357 in HA and 1.24 in A- has…

A: Buffer solution is made of weak acid and it's conjugate base or weak base and it's conjugate acid.

Q: Calculate the pH of hydrolysis of 0.500M NaF in water. (Ka=8.1x10^-4)

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: . Diethyl amine, (CH3)2NH, has a Kb of 5.81x10-4 at 25 C a. Write the dissociation reaction b.…

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.