A 0.050 M concentration of weak base, CH​3CH​2NH​2, was found to ionize at 1.7%. What is the concentration of CH​3CH​2NH​3+ in the solution?

Q: What is the pH of a solution prepared by mixing 25.0 mL of 0.180 M HC,H30, with 40.0 mL of 0.250 M…

A: pH of the solution = 13.71

Q: For a solution of 0.020 M lactic acid, HC3H5O2 (Ka = 8.4 × 10-4), calculate: [H+]= _______ M pH=…

A: For a weak acid ,HClO                     HC3 H5O2       ⇌      C3 H5O2 -       +      H+…

Q: In the laboratory, a general chemistry student measured the pH of a 0.345 M aqueous solution of…

A: The ionization reaction for caffeine is as follows, C8H10N4O2+H2O→HC8H10N4O2++OH- For above…

Q: Calculate the pH of a solution containing 0.0441 M potassium hydrogen fumarate and 0.026 M…

A: In the given question we have to calculate the pH of Solution,

Q: Vhat is the pH of a solution containing 0.2 M citric acid (pKa = 5.4) and 0.1 M sodium citrate?

A: Introduction: Since having sodium citrate that is a buffer solution so we can use the…

Q: A solution is made by dissolving 35.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Ba(NO2)2 is a salt which is mixture or strong base or weak acid so use pH of salt formula to get…

Q: Two acids are mixed in solution: 0.20 M of HBr and 1.50 M of HBRO (Ka = 2.3 x 10-9). What is the…

A: HBr is a strong acid while HBrO is weak acid and therefore, the resulting pH will be due to HBr,…

Q: A solution is made by dissolving 26.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Given that, Weight of Ba(NO₂)₂  = 26.5 g Weight of Ba(NO₂)₂  = 26.5 g/261.337 g/mol = 0.1014 mol…

Q: | Calculate the pH of a solution which is 0.345 M NHẠCI. (Kô of NH3 = 1.80 x 105)

A: Introduction: An acid is defined as substance which can donate protons and base which can accept…

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 0.00 ml of 0.150 M HBr?

A: Volume of KOH=50 mL  Concentration of KOH=0.150 M  Volume of HBr=0mL Concentration of HBr=0.150M

Q: What is the pH of (i) 1.0 X 103 M HBr and (ii) 1.0 X 102 M KOH?

A: We know that, pH and pOH can be expressed as the negative logarithm of hydrogen ion and hydroxide…

Q: 0.1 M Na2CO3 solution, using the given pH data, write expression for equilibrium constant (Ka or…

A: As the pH of Na2CO3 is 11.0 which means that it is basic in nature.

Q: Acid strength decreases in the series HI > HSO4 > HF > HCN. Which of these equal molar salt…

A: Solution: We know as pH increases basic nature of compound increases. The pH of any salt depends on…

Q: If 0.090 mole of solid NaOH is added to 1.0 liter of 0.180 M CH;COOH, what will the pH of the…

A:

Q: If a buffer solution is 0.150 M in a weak base (K, = 3.5 × 10-5) and 0.430 M in its conjugate acid,…

A: The Henderson- Hasselbalch equation can be used for the for the evaluation of pOH of the buffer…

Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

A: The question is based on the concept of PH calculations. we have been given a weak acid and its…

Q: If a buffer solution is 0.300 M in a weak acid -5, (K = 2.6 x 10) and 0.470 M in its conjugate base,…

A: The Henderson-Hasselbalch equation is given as,

Q: In the laboratory a student measures the percent ionization of a 0.532 M solution of benzoic acid,…

A: Given: Initial concentration of benzoic acid = 0.532 M percent ionization = 1.05 %

Q: Fill in the left side of this equilibrium constant equation for the reaction of carbonic acid…

A: in this question given ka ka= Acid dissociation constant, acid dissociation constant is used to…

Q: What is the pH of a buffered solution that is 0.12 m lactic acid (HC3H5O3) AND 0.10 m sodium…

A:

Q: Determine the pH of 0.500 M NaA solution if the Ka of HA is 4.0 x 10 (Hint: Base in water)

A: Given : Concentration of NaA = 0.500 M And Ka of HA = 4.0 X 10-9  Since A- (coming from salt NaA) is…

Q: Consider a mixture of 1.68 M HCIO and 2.12 M NaCIO. Given that the Ka for HCIO is 2.9x 10-8,…

A:

Q: A 0.050 M concentration of weak base, CH3CH2NH2, was found to ionize at 1.7%. What is the…

A: Interpretation: A 0.050 M concentration of weak base, CH3CH2NH2, was found to ionize at 1.7%. The…

Q: 1. What is the pH of a water that contains 120 mg/L of bicarbonate and 15 mg/L of carbonate ions?

A: Given: Concentration of bicarbonate i.e. HCO3- = 120 mg/L. And concentration of carbonate i.e. CO32-…

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 50.00 ml of 0.150 M HBr?

A: Volume of KOH=50 mL  Concentration of KOH=0.150M  Volume of HBr=50 mL  Concentration of HBr=0.150 M…

Q: 0.1 M NH4CI solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):

A: Net ionic reaction for the hydrolysis reaction in NH4Cl is given below NH4+​​​​​​​(aq) +…

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 15 ml of 0.150 M HBr?

A: Given  Volume of KOH = 50 ml = 0.050L Molarity of KOH = 0.150 M Volume of HBr = 15 ml = 0.015 L…

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: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 55.00 ml of 0.150 M HBr?

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration of a solution expressed…

Q: [4} What is the pH of the solution in the flask after 25.00 mL of 0.110 M NAOH has been added to…

A:

Q: Calculate the pH of 0.10 M Zn(NO3)2, which dissolves to give 0.10 M Zn2+ (pKa=9.0) and 0.20 M NO3-

A: Here we have to calculate the pH value.

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: 20 ml of 0.2 M NaOH solution be treated with 40 ml of 0.2 M acetic acid solution to give 60 ml.…

A: An acidic buffer is defined as an aqueous solution that consists of a mixture of a weak acid and its…

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: If 26.5 mL of 4.7 ✕ 10-4 M HI is added to 35.0 mL of 4.4 ✕ 10-4 M KOH, what is the pH of the…

A: Given :  Volume of HI (V1) = 26.5 mL Molarity of HI (M1) = 4.7 × 10-4 M Volume of KOH (V2) = 35.0 mL…

Q: A 0.581 M solution of a weak base has a pH of 11.86. What is the base hydrolysis constant, Kh, for…

A:

Q: 0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution…

A:

Q: A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the…

A: For NH3 , pKb = -log Kb = -log ( 1.86 x 10-5 ) = 5 - log 1.86 = 5 - 0.27 = 4.73 Concentration of…

Q: A 0.861 M solution of a weak base has a pH of 11.80. What is the base hydrolysis constant, K, for…

A: Hydrolysis constant Kb can be calculated by the following way .

Q: Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 MBa(OH)2 with…

A:

Q: What other species are present (in smaller amounts) in a 1.0 M hydrofluoric acid solution?

A: Concept - Hydrofluoric acid is amphoteric acid. So it can be ionized by giving H+ ion and it can…

Q: 4. You are given 1.500 M of HC1O,, Ką = 1.1 × 10² at 25°C. Determine its pH.

A: SOLUTION: Step 1: Since HClO2 has a low Ka value, it is a weak acid. Weak acids partially dissociate…

Q: If a buffer solution is 0.260 M in a weak acid (K, = 5.3 × 10-5) and 0.470 M in its conjugate base,…

A: This question is based on the prior knowledge of the Handerson Hasselbach equation which determines…

Q: 4. A weak base, B, is 1.2 % ionized in 0.20 M solution. What is Kb for B?

A: Suppose BOH is the weak base and it dissociate as:

Q: 125 mL of 0.3 M HC1 was mixed with 320 mL of 0.15 M NaF. What is the pH of the solution after…

A: Given data : Concentration of HCl = 0.3 M Volume of HCl = 125 mL Concentration of NaF = 0.15 M…

Q: If a buffer solution is 0.260 M in a weak acid (Ka=2.4 •10^-5) and 0.560M in its conjugate base,…

A: Given : Concentration of weak acid = 0.260 M Concentration of its conjugate base salt = 0.560 M And…

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.