Calculate the pH of a 0.50 M aqueous solution of HF. (K₂ 7.2 x 104) A. 3.6 x 10-4 B. 0.019 C. 1.7 D. 3.4

Q: A solution containing a mixture of 0.86 M  C2H5NH2 and a salt that has a common positive ion has a…

A: The dissociation reaction of C2H5NH2 is given by  C2H5NH2 (aq) + H2O (l) -------> C2H5NH3+ (aq) +…

Q: The following solutions were prepared: Solution A: 0.01 mole of perchloric acid (HClO4) dissolved…

A: Given- Moles of HClO4 = 0.01 Volume of water = 1L Moles of ethylamine hydrochloride = 0.01  Volume…

Q: . Which of the following solutions the has the lowest pH? A. 0.50 M HNO₂ (Ka = 4.6 x 10-4) B. 5.00 M…

A: Answer:- This question is answered by using the simple concept of calculation of pH of weak acids…

Q: A solution was found to have a pH of 13.33 at 25 °C. What is the concentration of OH? O a. 0.21 M O…

A: To find the OH- concentration, first find out the pOH and using that pOH, find out concentration of…

Q: The K a of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10 -4. What is the pH of a 0.20 M aqueous…

A: Given, the Ka for hydrofluoric acid =6.8×10-4concentration of HF =0.20 Mwe are asked to calculate…

Q: 1. Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous…

A: Given : Kb = 4.4 × 10-4 Concentration of methylamine = 0.20 M

Q: A 0.432 M solution of pyridine has a pH of 9.40. What is the K, of pyridine? Oa. 2.7 × 104 Ob. 1.5 x…

A:

Q: The pOH of a solution 5.50 M is 5.50. What is its hydroxide-ion concentration? 3.2 x 10-5 M 3.2 x…

A: POH of solution are as follows:

Q: What is the pH of a solution with [H3O+] = 3.9 x 10-6M?

A: Given :-  [H3O+] = 3.9 x 10-6M  To be calculated :- pH of the solution

Q: Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2b. 0.265 M NH4NO3…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: 9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? d. 3.2…

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

Q: What is the pH of 0.630 M CH3NH2Cl solution? (kb of CH3NH2 = 3.45 x 10-5) A. 9.13 B. 4.10 C. 5.75 D.…

A: NOTE : The formula of salt will be CH3NH3Cl. Since the salt will exist as ions CH3NH3+ and Cl- in…

Q: From what acid and what base are these salts below made from? a. Ca(NO3)2 b. NH4Br c. BaCl2

A:

Q: A 0.050 M solution of sodium meta-toluate (NaTol) has a pH of 8.47. a. What is the Kb of…

A: 0.050M sodium meta-toluate has a pH of 8.47. Kb and Ka is to be found. Sodium meta-toluate is a salt…

Q: A solution which is formed by combining 300 mL of 0.020 M NaOH with 700 mL of 0.010 M HCl has a pH…

A:

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

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

Q: Butyric acid is responsible for the odor in rancid butter. A solution of 0.25 M butyric acid has a…

A: Given that,The concentration of butyric acid,The pH of the solution = Ka for the acid = ?

Q: a. A solution of HNO3 has a pH of 3.69. What is the molarity of the solution? Molarity |M b. A…

A: We know that, HNO3 is strong acid. So, it is completely dissociated. Thus,  pH= -log[H+] Thus,  [H+]…

Q: Butyric acid (HC4H7O2) is responsible for the odor in rancid butter. A solution of 0.25 M butyric…

A:

Q: Four bases are prepared as 0.100 M aqueous solutions, which is the weakest base with the lowest pH?…

A: Kb is dissociation constant. It measures how completely a base disoociates into components ion in…

Q: a. A solution of HINO, has a pH of 3.57. What is the molarity of the solution? Molarity = M b. A…

A: pH = -log[H+]  Log [H+] = -pH  [H+] = 10-pH

Q: 1. Calculate the pH of the following: a. A solution whose pOH = 5.73 b. 12.0 M HNO3 c. 0.076 M…

A: Calculate the pH of the following---

Q: 5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this…

A:

Q: alculate the pH of a solution of 0.100 M Na2SO3. Ka1 = 1.23 x10-2 ; Ka2= 6.6 x 10-8 A. 4.55 B. None…

A: Sodium Sulphite (Na2SO3) is regarded as the fully deprotonated form (SO32-) of diprotic acid H2SO3.…

Q: What is the pH of a 0.379 M solutiôn of roxyla a. 0.42 b. 5.96 с. 3.19 O d. 6.38 O e. 4.2 x 10-7

A: Given, Molarity = 0.379 M Ka = 1.1 x 10-6  PH= ?

Q: Calculate the pH of each of the following strong acid solutions.   A. 5.55×10−2 M  HNO3. Express…

A:

Q: Calculate the pH of 0.65 M of a weak acid HA with Ka=2.56 x 10^-5 a. 5.59 b. 2.89 c. 2.78 d.…

A:

Q: . A 0.01 M aqueous solution of __________ will have a pH of 7.0 (neutral) at 25.0°C. a. NaOCl b.…

A: There is a concept that  When a salt of weak acid and strong base is hydrolyzed then pH of solution…

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

A: The concentration of weak acid, hypoiodous acid, HOI = 0.785 M The value of equilibrium constant for…

Q: The Ka for a weak acid is 1.2*10^-8. a. What is the equilibrium concentration of OH- in a 0.0020 M…

A: Given, Ka for a weak acid = 1.2 × 10-8 Molarity of its conjugate base = 0.0020 M   Let the weak acid…

Q: H 3PO 4 + H 2O  H 3O +1 + H 2PO 4 -1 What is the pH of a solution whose H +1 concentration is 4.0 X…

A: Conjugate acid-base pairs are those compounds which are differ by H+ ions.

Q: Calculate the pH of a 0.50 M aqueous solution of HF. (K₂ 7.2 x 104) A. 3.6 x 10-4 B. 0.019 C. 1.7 D.…

A: Concept:  We have weak acid ,which undergo weak dissociation so at equilibrium we can use the…

Q: of

A: Here HClO4, can't be made buffer solution because it is an strong electrolyte ( means strong acid )…

Q: a. 35 mL of 0.15 M H₂SO4 is mixed with 35 mL of 0.30 M NaOH O The pH of the solution is less than 7.…

A: pH is the measure of acidity or basicity of a solution. A solution with pH higher than 7 is basic…

Q: 7. A 0.6745-gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization.…

A: Since, Molarity is the number of moles of solute dissolve in one litre of the solution. Thus,

Q: Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 100.0 mL of 0.20 M…

A: We have 200 ml of weak acid of 0.3M We have 100 ml of 0.2 M of KClO We have to calculate the pH of…

Q: °C. What is the concentration of LIOH?

A: Given : pH = 13.14

Q: A 0.121 M solution of acetic acid has a pOH of 11.20. What is the K3 of acetic acid? Oa. 2.5 x 106…

A: Given: The concentration of acetic acid is 0.121 M The value of pOH is 11.20

Q: The k A.

A: