Given a weak base, B has Kb= 4.0 x 10^-6. Consider a 0.0020 M solution of the base.  a. calculate pOH b. calculate [H_30+] c. calculate Ka of the conjugate acid

Q: а. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where: H2Stag) > H*(ag) + HS…

A: pH is defined as negative logarithm of hydrogen ion concentration and it is represented as  pH =…

Q: Consider the Ka information to answer parts a-b. Ka 7.2 x 10 * K 4.2 x 10- Formula Kat 6.3x 10 a.…

A: Answer:- This question is answered by using the simple concept of calculation of Ka and Kb value…

Q: Consider a weak acid "HA". What is the pH of a 0.626 mol L¯' solution of HA? The KA of HA is 6.5 x…

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Q: The weak acid HZ has a Ka of 2.55 x 10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: The following reactions all have K < 1. 1) CIO (aq) + CGH;OH (aq)= HCIO (aq) + C,HsO (aq) 2) НСОО…

A: We need to arrange the given ions and compounds according to their base strength.

Q: HX (M = 150. g/mol) and HY (M = 50.0 g/mol) are weak acids. A solution of 12.0 g/L of HX has the…

A: Given data: The molar mass of HX = 150. g/mol. The molar mass of HY = 50.0 g/mol. The mass of HX =…

Q: A weak base, B, has Kb = 4.0X10^-6. Consider a 0.0020 M solution of the base.  a. Calculate pOH b.…

A: Suppose the weak base be A-. It gets hydrolyze according to the equation: A- + H2O &lt;----&gt; HA +…

Q: What is the pH of a 0.20 M solution of a generic weak acid? The Kb value for this generic weak acid…

A: Given data  kb = 4.0 x 10-5 concentration, c= 0.20 M Formula used       OH- = kb×cpOH =…

Q: 3. In the reaction below, H2O is a(n): H2SO; +H2O → H;O*+ HSO; a. Base b. acid Su conjugate acid d.…

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

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: What is the pH (aq., 25 oC) of 30.00 mL of a 0.250 M HBr solution that has had 15.00 mL of 0.125 M…

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Q: Find pH of a 0.1M solution of HOAc  (ka=1.78x10^-5) with 0.1M NaOH

A: When NaOH is added to aceticacid (HOAc) NaOAc salt is formed             HOAc            +    NaOH…

Q: Calculate the value of H,O* from the given [OH] in each solution and label the solution as acidic or…

A: pH  =  - log [ H3O+ ]  [ H3O+ ]  = 10-pH     pOH  =  - log [ OH- ]  [ OH- ]  = 10-pOH      pH  +…

Q: 1    Calculate the pH of a 0.02 M solution of the weak acid, HA.         Ka = 2.46 X 10 –4…

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Q: Calculate the pH of an aqueous solution at 25°C that is 6.2x 10 3 M in HI. pH

A: Given: Concentration of HI=6.2×10-3M To find: pH

Q: Butyric acid  ( C3H7COOH) is a weak acid . What is the pH of a 0.0250 M solution of this acid. Ka =…

A: For weak acids, ions dissociation is very small that results in small H+ ions amount. Their…

Q: A friend of yours has to find the pH of a 1.0 x 10-8 M hydrochloric acid at 25˚C. Your friend notes…

A: Here concentration of acid(HCl) is very very less(i.e. solution is diluted). Hence, the…

Q: Calculate the pH of solution made by combining 100 ml of 0.28 M HC,H;O2 and 50 ml of 0.36 M NaOH, Ka…

A: Since there is mixing of weak acid and strong base so it is a case of acidic buffer. The pH can be…

Q: The weak acid HZ has a Ka of 2.55x10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Given: Ka for HZ = 2.55 x 10-4 Since HZ is a weak acid, it will not get dissociated completely into…

Q: A weak acid HA has a Ka of 5.3x10-5. A solution of HA has a pH of 3.00 a) Calculate the initial…

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Q: A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA…

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Q: A solution is prepared at 25oC that is initially 0.42 M in a “X” base, a weak base with Kb =…

A: Since the solution is having base X with concentration 0.42 M and its conjugate acid salt with…

Q: The pH of a 0.1 M solution of a monobasic acid P is 1.0 while the pH of a 0.2 M solution of another…

A: Here we have to explain the properties the two monobasic acid P and Q . Given - The pH of 0.1 M P is…

Q: Calculating the A solution is prepared at 25 °C that is initially 0.13M in acetic acid (HCH,CO,), a…

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Q: 7. Consider an HCI solution of concentration 4.25x10"M a. [4] Find the pH b. [4] Find the pOH ~log…

A: The concentration of the given HCl solution is = 4.25×10-4 M a. The pH of solution =? b. The pOH of…

Q: A solution is prepared at 25 °C that is initially 0.14M in propanoic acid (HC,H,CO,), a weak acid…

A: Given :-  Concentration of propanoic acid = 0.14 M  Concentration of potassium propanoate = 0.012 M…

Q: HA, a weak acid, also forms the ion HA2- in solution. The reaction is HA(aq)+A−(aq)↽−−⇀HA2-(aq)…

A: The ratio of moles to volume is known as concentration.

Q: Calculate the pH value of 0.00 * ? acid at 25 C if Ka=0.0O00018 3.1

A: Given:  0.001M acetic acid at 25C if Ka = 0.000018   To find: pH value of 0.001M acetic acid at 25C…

Q: Find the pH of each mixture of acids. 0.105 M in formic acid and 5.5×10−2 M in hypochlorous acid

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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: Kb value for given weak base is 5.2×10^-5.

Q: 7. Carbonic acid (H2CO3) is a diprotic acid with Ka1 = 4.30 × 10–7 and   Ka2 = 5.60 × 10–11 What…

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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

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Q: OH–

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Q: Find the a0 and a1 values ​​of hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10^-8 for…

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Q: A 1.50 g sample of lithium nitrite, LiNO2, is added to 100.0 mL of water. Acid dissociation constant…

A:

Q: The diagrams here show three weak acids HA (A = X, Y, or Z) in solution.  (The hydrated proton is…

A: Given, Three acids HX, HY &amp; HZ. Hydronium ion is shown in figure (red).

Q: Find the pH of a solution prepared by dissolving 12.43 g tris (121.136) plus mol' 4.67 g tris HCI…

A: Given: Mass of tris = 12.43 g Mass of tris HCl = 4.67 g Molar mass of tris = 121.136 g/mol Mass mass…

Q: Which statement is true? I  If a solution has a pH of 12.0, there are more H+ ions in this solution…

A: 1) Since the pH of pure water = 7  And since pH = -log[H+] where [H+] = concentration of H+ ions…

Q: 4) A solution is created by measuring 3.60 x 10-3moles of NaOH and 5.95 x 10-4moles of HCl into a…

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: pH pOH [H*] [OH] Acidic or basic? a. b. С. d. 10.4 e. f. g. h. 5.3 i. k. I. 3.5 x 104 m. n. o. р.…

A: The relationships which we will be using are, 1) pH = -log[H+ ] 2) pOH = -log[OH- ] 3) pH + pOH = 14…

Q: A 0.175 M weak acid solution has a pH of 3.25. Find Ka for the acid.

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Q: Calculate the pH of each solution at 25 °C and indicate whether the solution is acidic or basic.(a)…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: 7. A 0.050 M solution of an organic acid has a [H*] = 5.9 x 103M. a) Calculate the pH of the…

A: We have given that  Concentration of organic acid [HA] = 0.05 M  [H+] = 5.9×10-3 M

Q: 1. Find the pH of 0.0500M CH¿CICOOH (a weak acid) where Ka=1.4 x 103

A: The PH of chloroacetic acid(CH2ClCOOH) can be calculated as follows

Q: 2. If we mix 0.50 mol NaOAc and 0.50 mol HCIO into 1-L solution, the resulting solution should have…

A: Given: Moles of NaOAc mixed = 0.50 mol Moles of HClO mixed = 0.50 mol Volume = 1 L Kb(OAc-) =…

Q: Ka = 5.0 x 1010 for formic acid, CHOOH. Given a 0.20 mol/L of this acid solution, calculate the…

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Q: e. Bi H₂O + MnO, Bi MnO + OH Bi+Minou-Biano + f. SOCIO; + OH H₂O SO,+ Chu 8. Cu + HNO, → Cu" + NO +…

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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?

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Q: A weak acid has K₂ = 1.00 x 103. If [HA] = 1.00 M what must be [A] for the pH to be 2.7? 0.50 M 2.0…

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Q: What is the pH of a solution obtained by mixing 0.59 L of 0.100 M  Ba(OH)2 and 0.10 L of 0.118 M…

A: Acid and base are the chemical compounds which upon adding in water change the pH value accordingly.…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.