9. If only 4.1% of 0.50 M solution of a weak base was ionized. Calculate its Kb value? * O 5.2 x 10* O 1.2 x 104 3.4 x 10 O 4.1 x 10* 8.8 x 10

Q: The weak acid, HA, has a Ka of 3.00 x 10-8. What is the Kb of its conjugate base, A"? 1.39x10-12 O…

A:

Q: 9. If only 1.6% of 0.20 M solution of a weak base was ionized. Calculate its Kb value? *

A:

Q: Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCI (C14H2NONH,CI). Note that lidocaine…

A: Since C14H21NONH is a weak base with pKb = 7.94 Hence the pKa of its conjugate base i.e C14H21NONH2+…

Q: Calculate the pH of a solution in which [OH-] = 2.50 x 10-14 M (A) -3.60 B) 10.40 3.60 13.60 E) 0.40

A: Given: [OH- ] = 2.50 X 10-14 M

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: Calculate the pH at 25 ° C of a 0.0033 M solution of a weak base with a Kb of 2.5 × 10−9 . pH =

A: Given:Kb = 2.5×10−9.Weak base [BOH] = 0.0033 M.

Q: 11. What is [H*] in M for a solution with POH=1 ]1 × 10–12 |1 x 10-7 1 × 10–13 |1 x 10-9 |None of…

A: PH is defined as negative logarithm of concentration of [H+] ion.

Q: The [OH-] = 1.3 x 10–6 M for a 0.025 M solution of a weak base. Calculate the value of Kb for this…

A: Consider the given information is as follows; OH- = 1.3×10-6 MConcentration of weak base BOH = 0.025…

Q: 1. A1.0 M solution of a weak base B has a pH of 11.60. What is the valve of Kb for this base? а. 6.3…

A:

Q: Consider HA (a weak acid) and HB (a weak base). 11) A 0.10 M solution of the weak base D has a pH…

A: Given: pH = 11.45 concentration of weak base = 0.10 M

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.186? 6.52 -…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The [H*] of a solution with pOH=4.3 is: O 3.2 x 10-4 M 4.3 x 10-5 M O 6.8 x 10-9 M O 1.99 x 10-10 M

A: We have given that pH : The pH of a solution is a measure of the molar concentration of hydrogen…

Q: I'm not sure how to solve this one

A: pH = -log[H+]  Since HCl will dissolve completely as per the reaction  HCl ----> H+ + Cl-  Since…

Q: Calculate the hydrogen ion concentration (in M) of a NaOH solution with a pOH of 4.23 . A)…

A: Given: pOH of NaOH = 4.23

Q: 28. What is the pH of a 0.62 M NH;NO3 solution at 25 °C? * [Kb for NH, is 1.76 × 10*] A. 2.48 В.…

A: Ammonium nitrate is a slat of weak base, ammonium hydroxide and strong acid, nitric acid.…

Q: Calculate the pH of 0.030 M Ba(OH), solution. 12.78 O 1230 O 122 O 12.48 12.16

A:

Q: Calculate the pH at 25 °C of a 0.36M solution of sodium hypochlorite (NaClO) . Note that…

A: Given: Concentration of NaClO = 0.36M pKa of HClO = 7.50

Q: The [OH-] = 1.3 x 10-° M for a 0.025 M solution of a weak base. Calculate the value of Kb for this…

A: Consider reaction for the weak base is as follows; Reaction:      BOH aq        +        H2Ol…

Q: Ka for ammonium, its conjugate acid. (NH4+) = 5.68 x 10^-10 Using the answer above, what is the pH…

A: Given: Ka = 5.68 x 10-10 Concentration of NH4Cl = 0.140 M

Q: 5.00 g NaOH and 5.00 g Ba(OH)2 were used to prepare 1L solution each. Which solution will be more…

A: Consider the given information is as follows; Mass of NaOH = 5.00 g Mass of Ba(OH)2 = 5.00 g Volume…

Q: The base protonation constant K, of lidocaine (C4H, NONH) is 1.15 x 10 °. Calculate the pH of a 0.55…

A: Given, kb = 1.15 * 10-8  Concentration of solution = 0.55 M Temperature = 25◦c

Q: The poison strychnine is a weakly basic compound with Kb = 1.8 x 10 What is the pH of a 0.058 M…

A: Given that, 0.058 M solution of a weak base, i.e. C = 0.058 M. The Kb is 1.8×10-6. We have to…

Q: Calculate the pH of 0.7 M of Aniline solution CeHgNH2 CeHgNH2 + H20 CeHgNH3 + OH K for Aniline = 4…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: The Kb value for methylamine, CH3NH2, is 4.2 x 10-4. What is the pH of an aqueous solution for which…

A: Here we are required to find the pH of methylamine

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.186? O 1.53…

A: Given: pH=4.186 [H+]=6.52×10-5 Formula used: pH=-logH+H+OH-=10-14

Q: Calculate the pH of a solution that contains 3.9 x 10 -5  M H3O⁺  at 25°C.     4.41     9.59…

A: Please find your solution below :

Q: weak Mandalorious acid (HMaO3): 4.5 x10-1 M, Ka = 6.7 x 10-5  Determine the pH of the solution

A: The acid dissociation constant for the HMaO3 is = 6.7×10-5 The concentration of HMaO3 solution is =…

Q: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…

A: Given,  for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 10.04. What is the Kb of this base

A:

Q: Calculate the pH at 25 °C of a 0.59M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A: Given-> Concentration of NaClO = 0.59 M pKa (HClO) = 7.50

Q: c. H20 = Lewis Base (donate 10. Calculate the pH of 0.3M solution of NH,Br if Ka of NH4* = 5.6x10-10…

A: The pH of a 0.3 M solution of NH4Br is to be calculated if Ka of NH4+ = 5.6×10-10

Q: A week diprotic acid H2A has Ka1 = 4.2 x 10-7 and K2 = 4.8 x 10-11. Determine the pH of a 0.17 M…

A: Whenever a weak diprotic acid and strong base reacts with each other than it form a salt which…

Q: Fill in the blanks: Ka of acetic acid is 1.80 x105 and that for hypochlorous acid is 3.0 x 108 The…

A:

Q: Determine the pH and the type of solution of a 0.227 g/L C5H5N solution at 25°C.  The Kb of C5H5N is…

A: At 25°C Concentration=0.227g/L Kb of C5H5N = 1.7 ×10^-9

Q: Calculate the pH at 25 °C of a 0.23M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A:

Q: The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M solution of…

A: Given: The amount of malonic acid dissolved in 0.250 L is 19.5 g. The pH of malonic acid and 0.300 M…

Q: 1.58 x10-M b) Ca(OH)2 Calculate pH of 0.1 M solution of a weak base with Kb = 1.65 x10-7 %3D P=3.89

A: Weak base is taken as B.An ICE table is constructed to determine the equilibrium concentration of…

Q: What is the concentration of hydroxide ion of 0.075 M NH3 solution. (Kb= 1.75 x 10-5 ). a) 1.58 x…

A: As ammonia is a weak base, hence it does not dissociate completely in water

Q: Determine the pH of a 0.588 M weak base soultions at 25C. The Kb for the weak base is 1.76 x 10^-5.…

A:

Q: For a certain acid pK 7.49. Calculate the pH at which an aqueous solution of this acid would be…

A: Given, pKa = 7.49 Dissociated= 0.15% Let us assume the acid dissociate reaction HA <=> H+ + A-

Q: The pH of an unknown monoprotic acid HA is 4.58. Its concentration is tested to be 0.575 M.…

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Q: Calculate the pOH of a solution that contains 3.9 × 10¬4 M H3O† at 25 °C. 9.59 10.59 0.59 3.41 4.41

A:

Q: 5. 5.00 g NaOH and 5.00 g Ba(OH)2 were used to prepare 1L solution each. Which solution will be more…

A: The mass of NaOH is = 5.00 g The mass of Ba(OH)2 is = 5.00 g The volume of solution is =1 L The…

Q: of

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

Q: Calculate the hydronium ion concentration (in M) of a blood sample with a pOH of 7.8. O 1.58x10-8 O…

A: Given pOH = 7.8

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: 7. A solution with pH of 9.50 has a pOH of А. 9.50 О В. О.50 Ос. 4.50 D 11 3

A: pH  is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions  are…

Q: For H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by…

A: Given,  Ka1 = 9.6×10-8 and Ka2 = 1.3×10-14

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.28. What is the Kb of this base?

A: