Determine [H30*] of a 0.250 M solution of formic acid (Ka 1.8 x 10-4).

Q: Calculate the ph of 1.55 M CH3NH2. The Kb for CH3NH2= 4.4 x 10^-4

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Q: MCQ 162: The ionic equation O+ H,O → 20H". This will result in an H A. acidic solution B. alkaline…

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Q: Calculate the pH of a solution with [OH-] = 2.0 x 10-11 M

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Q: 37. Compute the concentration of hydroxide ion, [OH] in 0.2 M HF. Given Ka for HF is 6.6 x 10-4. * O…

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Q: 0.92 M

A: From Henderson equation we know that    pH = pKa + log [salt] / [acid ]   ............ (1)

Q: a) Determine the pH for the following solution: [OH−] = 1.6×10^−5 M  b) Is the above solution…

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Q: Calculate the pH of 4.0 X10*-4 M KOH O a. 9.40 O b. 3.40 O c. 4.60 Od. O d. 10.60

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Q: Calculate the pH of a 3.39×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

A: Given : Concentration of NaF = 3.39 X 10-3 M And Ka of HF = 6.80 X 10-4  Since the salt NaF contains…

Q: A diprotic acid (H₂A) has Kal = 4.28 x 10-7 and K₁2 = 5.45 x 10-¹1. What is the pH of a 0.431 M H₂A…

A: Firstly we find the concentration of H+ ion. Then we find the pH. Shown in step 2.

Q: Amphetamine (C,H13N) is a weak base with a pKp of 4.2. Part A Calculate the pH of a solution…

A: 1-Phenylpropan-2-amine is amphetamine. Its molecular mass (M) is 135.23 g/mol Concentration of…

Q: Rank the following in order of most acidic to least acidic. Solution X pH = 8.50 %3D A) Z > X > Y B)…

A: pH is defined as power of hydrogen.  PH = -log(H +)

Q: Rank the following solutions from th A. 1.2x10-5 M NaOH 9.07 В. О.0015 М HCI С. О.13 М НF D. 7.1x107…

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Q: Acetic acid has a Kₐ of 1.8X10⁻⁵, and ammonia has a K(b) of 1.8X10⁻⁵. Find [H₃O⁺], [OH⁻], pH,…

A: (a) The acetic acid is a weak acid. The weak acid does not fully dissociate into its ions. We need…

Q: Calculate the pH of 4.0 X10^-4 M KOH O a. 4.60 b. O b. 3.40 c. O c. 9.40 O d. 10.60

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Q: 6. Pyridine (P), a pesticide, is a weak base. Calculate the pH of a 0.0030 M solution of this base.…

A: In the given question we have to calculate the pH of Solution,  the Reaction of weak base,  C5H5N  +…

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: Calculate the pH of a 0.0250 M solution of butanoic acid. Ka = 1.5x10-5 HC4H7O2(aq) +H2O(l) = H3O+…

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Q: What is the pOH of a solution that has a H3O+ concentration equal to 8.23 x 10-5 M at 25°C?

A: The sum of pH and pOH is equal to 14.  So from pOH value also we can know that the solution is…

Q: Find the concentration of H+ ions in these situations: a.) a strongly acidic solution where [OH-] =…

A: (a) [OH-] = 1.0 × 10-12 M  We know at room temperature (25°C); [H+] × [OH-] = 10-14 [H+] × (1.0 ×…

Q: Calculate the pH at 25 °C of a 0.71M solution of sodium hypochlorite (NaCIO) . Note that…

A: NaClO dissociates into Na+ and -OCl.  NaClO(aq)→Na+(aq)+OCl-(aq)OCl-(aq)+H2O(l)→HOCl(aq)+OH-(aq)

Q: Determine the Kb of a weak base that has a concentration of 0.75 M and a pOH of 4.74 at 25°C.

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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: Find the pH of a 0.0237 M benzoic acid (C6­H5COOH) solution. The Ka of benzoic acid is 6.28 x 10-5…

A: Given:

Q: please highlight the correct answer

A: Relationship between [H3O+] and [OH-] is, For a neutral solution,

Q: Calculate the pH at 25 °C of a 0.20 M solution of sodium hypochlorite (NaCIO) . Note that…

A: The pH of the solution has to be calculated

Q: show ur work(calculation) and answer properly

A: We are given a weak base, it's concentration and percentage ionisation is given. We have to find kb.

Q: What is the [H3O+] in a solution with [OH-] = 4.0 x 10-6M?

A: Since the pH of any solution is given by  pH = -log[H3O+ ]  where [H3O+ ] = concentration of H3O+…

Q: Calculate the ratio [CH3COOH] / [NaCH3CO0] that gives a solution with pH = 5.00 (Ka CH3COOH = 1.8 x…

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Q: 2. Answer the questions for the acid below: HA(aq) + H20(1)→H30* (aq) + A-(aq) a) Write the acid…

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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: 16.) A sdution od 8.m g 88.0M unt is othe Ko f a We ak acid, HA, is 0.47% ranized. the Weak acid.…

A: The molarity of given weak acd, HA =8.0 M As HA is a weak acid, it dissociates partially into A- and…

Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.

A: Concentration of Al ion = 0.064 M

Q: If your pH = 3.4, find pOH O 1.0 O 70 O 10.6 O 1.0x 10

A: The solution is as follows :

Q: How much mL of BaSO4 will be recovered given the following: Solution A: Na2SO4(aq) = 0.01 M; V =…

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Q: Calculate the pH of a 0.20 M KH2AsO4 solution (H3AsO4   Ka values: Ka1 = 5 x 10^-3 , Ka2 = 8 x10^-8…

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

Q: What is [H30+] in a solution with [OH-] = 8.0 * 10^-5 M?

A: The pH of solution indicates the number of H+ ions in the solution. The pH scale ranges from 0 to 14…

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

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Q: Calculate the Ka of a 0.400 M acid solution with [H 3 O^ + ]=1.4*10^ -4 M

A: Given,  The concentration of an acid =0.400 M.  and the [H3O+] = 1.4×10-4 M

Q: Calculate [H+], PH and POH respectively of CH3COOH solution has concentration 1.0 x 10-3 M and the…

A: Here i have calculated all the things

Q: 3. What is the pH in a solution with [H*]=2.5x10-5? %3D

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Q: An acid with a ka = 2.3 x 104 has a conjugate base with kb of O 1.0 x 10-14 O 1.4 x 10-5 4.3 x 10-11…

A: There is relation between Ka and Kb , Ka × Kb = Kw  Kw = ( Ionization constant of water ) = 1.0 ×…

Q: Calculate the pH of a 0.20 M solution of NH4NO3 Kb(NH3) = 1.8x10^-5 Thank you :)

A: A pH scale is a scale that is used to determine the acidic and basic nature of a solution. If the pH…

Q: The Ka of hypochlorous acid (HCIO) is 3.0 x 103 at 25.0 °C. Calculate the pH of a 0.0335 M…

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Q: Calculate the pH of 0.050 M aqueous solutions of the compounds below at 25 °C: a. NaOH b. CH3NH2…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: What is the pH of a 0.844 M solution of hypochlorous acid (Ka 2.9 x 10-8)?

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Q: Morphine (C17H19O3N) (MM 285.34) is a weak base with a kb of 7.4 x 10-7. Calculate the pH of a…

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Q: Calculate the pH at 25 °C of a 0.47M solution of anilinium chloride (C,H;NH,CI). Note that aniline…

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Q: What is the pH of a solution of 0.20 M HNO2 containing 0.10 M NaNO2 at 25 °C. The Ka of HNO2 is 4.5…

A: pH of a solution tells about the nature of the solution whether it is acidic or basic. The values on…

Q: Calculate the pH of a 0.41 M CH3COONa solution. (Ka for acetic acid = 1.8 ×10−5.)

A: The reaction is written below. CH3COO - + H2O ⇌ CH3COOH - + OH- The ICE table is shown below.

Q: What is Ka for the conjugate acid of NH₃ (Kb = 1.8 × 10⁻⁵)?

A:

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.