ame pH, or not? xplain why this is so.

Q: The pH of a basic solution is 12.17. What is [H]? M 3 4 6. C 7 8 +/- x 100

A:

Q: A solution is made by dissolving 0.0015 mole Ba(OH)2 in enough water to make 1.50 liter of solution.…

A: Given- Moles of Ba(OH)2=0.0015mol Volume of solution=1.50L  pH=? pOH=?

Q: Calculate the pH of a solution that is 0.210 M nitrous acid (HNO₂) and 0.290 M potassium nitrite…

A:

Q: The percent ionization of a 0.10M weak acid is 0.0036%. Calculate the pH of the solution and the Ka…

A: Given a weak acidconcentration = M = 0.10 M% ionization = % = 0.0036%pH of solution = to be…

Q: when the pH of a solution containing 15mL of 0.10 M CH3COONa and 10 mL of 0.10M CH3COOH (pKa=4.74)?…

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Q: What is the hydrogen ion concentration in a solution with pH 8.64? (2.3x10-9M or 0.0000000023 M)

A: Answer

Q: The pH of 8.35 is wrong, but I'm not sure how to get the right answer

A: 17.3 mL of 0.130 M H2CO3 solution is titrated with 0.0776 M KOH solution.We have to calculate the…

Q: Natalie a new lab technician needs training on how to determine molarity and pH/pOH of a solution.…

A: We have to explain the steps needed and show her how to calculate the pH/pOH anddetermine if the…

Q: 16. What is the pH of 10.0 mL of 0.0020 M HCI? ALQ.70 B) 2.70 C) 3.70 D) 5.70 E) 10.0 17. The pH of…

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Q: 10:55 AM Wed Jul 5 Question 10 of 15 1 4 7 +/- Tan here or pull up for additional resources The pH…

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Q: An unknown weak acid with a concentration of 0.590 M has a pH of 5.600. What is the Ka of the weak…

A:

Q: What is the factor difference between a solution with a pH of 9 and 9.3?

A: Given: Initial pH = 9  Final pH = 9.3

Q: How many milliliters of 0.100 M HCIO3 are required to neutralize 48.0 mL of 0.140 M KOH?

A:

Q: 11. Calculate the pH of a .0275 M orange juice solution (Ka citric acid 1.1 x 10-3).

A: Given  Concentration of acid = 0.0275 M  Ionization constant of citric acid ( Ka ) =  1.1 × 10-3  PH…

Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO¯ and 0.41 M in HIO? The Ka for HIO is 2.3…

A: 1- First calculate the pKa value of acid HIO :  We know that, pKa = -log(Ka)  pKa = -log( 2.3 ×…

Q: Question 1

A: Given: A buffer is prepared by mixing 50.0 mL of 0.101 M nitrous acid and 22.0 mL of 0.105 M NaOH.

Q: how do you counstruct a pH curve for a triprotic acid? For example 75.00 mL of 0.137 M H3PO4 with…

A: The acid dissociation constants for phosphoric acid are quite different from each other with pKa's…

Q: A beaker contains 10.888 mL of a 0.111 M solution of CSOH. This is titrated with 13.81 mL of a…

A: Given that, 10.888 mL of 0.111 M CsOH is titrated with 13.81 mL of 0.0271 M HNO3. We have to…

Q: 6:15 1 An unknown weak acid with a concentration of 0.074 M has a pH of 1.80. What is the Ka of the…

A: Given pH = 1.80 Concentration = 0.074 M

Q: Calculate the pH of a solution that is 2.3 x 10-4 M in HNO3. 32 64 43 36 none of the above

A: pH of Solution: It measures the hydrogen ion concentration in solution, which helps in the acidity's…

Q: If you had 98 ml of a 0.60M solution of HCN that you mixed with 110 ml of a 0.50M solution of KOH,…

A: Solution : pH       pH is a quantitative measure for the acidity or basicity of the solution. This…

Q: QUESTION 3 A solution was prepared by dissolving 2.76g KOH in 687 mL of 0.0983M Mg(OH)2. What is the…

A: Answer :- b) 13.428

Q: 2. Calculate the volume, in milliliters, of a 0.390 M KOH solution that should be added to 5.50g of…

A: In given question buffer is prepared from strong base KOH and weak acid HEPES. We will use Henderson…

Q: What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK? Ka of HCOOH is 1.7 x 10-4…

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Q: The pH of an aqueous solution of 0.569 M quinoline (a weak base with the formula CoH7N) is Submit…

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Q: 14. What is the pH of a 2.58 M solution of ZnCl(aq)? (K,-1.0 x 10 for Zn(H₂O),"") 5.59 11.71 4.29 d.…

A: Concentration of ZnCl2 (aq) = 2.58 MKa = 1 x 10-9 We have to calculate the ph of the resulting…

Q: What volume (in mL) of 9.2 M HCIO4 would be required to make 500.0 mL of a solution with a pH of…

A: The pH of a solution is represented by the following relation: pH=-log[H+] Where [H+] is the…

Q: The pH of a basic solution is 11.27. What is [H*]?

A: pH = 11.27  [H+] = ?

Q: You are given a 0.25 M solution of an unknown weak base. Use 1/10th of dilution to find unknown weak…

A: In the given solution we are provided with 0.25 M solution of an unknown weak base which is then…

Q: O Aind the Concentiation A HaO in a O,250M Ihadirofuaric Oad (HF) soutione the Ka kr HFIS 3.50 104…

A: Since, HF is a weak acid. Weak acid is the one which undergoes partial dissociation. The…

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.