What is the pH of a solution that is 0.03M in picric acid and 0.1M in sodium picrate. pka=0.38 O a. 1.7 O b. 5.9 O c. 1.83 O d. 0.9

Q: A) 0.0956 g ammonium chloride, and made 50.0 mL of solution, what would the initial pH of this…

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

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: 4. Which solution has the lower pH? a. 0.1M HCl or 0.1M HC2H30₂ b. C. 0.1M NaOH or 0.1M NH3(aq) 0.1M…

A: We have find out the answer.

Q: What is the normal pH of blood? a. =7.0 Ob. =5.1 O C. -7.4 O d. =14.0

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Q: The pH of a 0.063 M solution of a weak acid is 3.95. What is the value of Ka for this acid. A. 2.5 x…

A: Interpretation: The pH of a 0.063 M solution of a weak acid is 3.95. The value of Ka for this acid…

Q: A solution is prepared by adding 0.10 mol of ammonium chloride, NH4Cl, to 1.00 L of water.  Which…

A: Salt formed from Strong acid + Strong base gives neutral solutiom Strong acid + weak base gives…

Q: A solution with a low pH means what? 1. A high number of hydrogen ions are in a solution 2. A basic…

A: We are to find out what does a solution with lower pH mean. We will consider the concentration of…

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

A: dExplanation:

Q: 1. For each of the salts (assume at this point completely soluble), write the equation for…

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Q: Which one of the following 0.1 M aqueous solutions has pH = 7?   A.  NH4NO3   B.  NaClO4   C.…

A: pH of 7 will only be given by a neutral solution.

Q: 28. Which acid has the lowest pH? 0.040 M HCI A. B. 0.020 M HCIO4 C. 0.050 M HNO, D. 0.030 M HBr

A: pH : pH can be defined as the negative logarithm of hydrogen ion (H+) concentration. The formula is,…

Q: What is the pH of a solution that is 0.150 M NH3 and 0.200 M NH4CI? Kb of NH3 = 1.8 x 10-5 O9.26…

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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…

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

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

Q: What is the pH of a 3.3 × 10-4 M CSOH solution?

A:

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: b. hydrogen ion d. hydride ion 4. In a laboratory activity, LIOH) is completely dissolved in…

A: Neutralization reaction - when acid and base reacts to form salt and water is called neutralization…

Q: Which solution will have the lowest pH (most acidic)? a. 0.10 M HCIO. b. 0.10 М НСIO с. 0.10 МКОН d.…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: 7) An aqueous solution of NaF is prepared by dissolving 0.250 mol of NaF in sufficient water to…

A: The objective of this question is to calculate the pH of a solution of sodium fluoride (NaF) at 25.0…

Q: What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN? (Ka = 4.9 x 1010…

A: Answer :- HCN is a weak acid and NaCN is its conjugate Salt . This solution is basically acts as a…

Q: This compound is a weak organic base: C18H21O3N + H2O C18H21O3NH+ + OH-…

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Q: The molar concentration of H+ ions in a solution is 5.8 x 10-9. The pH is a. 9.00 b. 5.80 c.…

A: pH can be calculated as pH = -log [H+]

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2?   a. 10.2   b. 2.0   c. 9.0   d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: a. What is the hydroxyl concentration of the ammonia solution? b. What is the pOH of the ammonia…

A: Given: Volume of ammonia solution= 300ml Concentration of ammonia solution= 0.05M The density of the…

Q: A 4.0 M HCl solution is used to titrate a 2.0 M KOH solution.   a.   How many ml of the HCl…

A: To  solve the question regarding neutralization reaction.

Q: Calculate the pH of a 1000 mL solution prepared by dissolving in water 0.600 mol of a weak acid HA…

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Q: Calculate the concentration of OH- in a solution that contains 6.5 x 104 M H30 + at 25°C. Identify…

A: A solution is acidic if pH<7 Basic if pH>7 pH = -log[H+] pOH = -log[OH-] pH+pOH = 14

Q: What is the pH of the solution when 50.0 mL of 0.10 M KOH and 50.0 mL of 0.12 M HCl are mixed?…

A: Given  HCl      +       KOH   ->    KCl   +   H2O 0.12M         0.10M 50ml            50ml  pH =…

Q: Calculate the pH of a solution that's 0.65M in NaF and 0.75M in HF. (HF. Ka = 7.2 x 10-4)? A.3.08…

A:

Q: Complete the reactions for dissolving the following two acids into water. Then, label the Acid,…

A: We have to predict acid base conjugate acid and bases in the given reactions.

Q: Calculate the percent ionization for a 0.200 M HCOOH solution.  Ka = 1.80 x 10-4. a. 5.91 b.…

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Q: What is the pH of a solution made of 0.15M NH3 and 0.23M NH4Cl? where the Kb= 1.8 x 10-5. A. 4.61…

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Q: Which of the solutions listed below has the lowest pH? A. Pure H20 B. 2.5 x 10° M HNO3 C. 0.10 M…

A: Given the solution have lowest PH from following solution a) pure H2O    b) 2.5 * 10^-5M HNO3…

Q: What mass of LIOH would need to be dissolved in water to make 300.0 mL of a solution with a pH of…

A: Given :- pH = 11.71               Volume of solution = 300.0 mL  To calculate :- mass of LiOH needed…

Q: Which of the following solutions would have the highest pH?  Assume that they are all 0.10 M in acid…

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Q: For each of the following substances, predict the pH when each is dissolved in water.  Is it basic,…

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Q: A 0.25 M solution of a weak monoprotic acid has a hydronium-ion concentration of 3.5 x 104 M. What…

A: Concentration of weak monoprotic acid, [HA]  =0.25M [H3O+] = 3.5 X 10-4  M

Q: An aqueous solution of a weak acid, HA is prepared by dissolving 0.030 mol of HA in water to yield…

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Q: Write net ionic equations for the reactions that take place when aqueous solutions of the following…

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

Q: What is the pH of IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: Calculate the pH of each solution. a. 1.0 M NaH2PO4 b. 1.0 M Na2HPO4

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Q: Arrange the following solution from lowest pH to highest pH:

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

Q: Calculate the pH of a 0.12 M solution of NaC2H3O2 (for HC2H3O2 Ka= 1.8 x 10 ^-5). A. 5.09 B. 8.91…

A: Answer:When salt of weak acid and strong base is added in water it gets hydrolyzed to produce OH-…

Q: Calculate the H3O+ and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

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Q: 1.0 x 10-11 moles of HCl are added to 1.OL of H20. What is the pH? О 3.0 O 10.0 O 11.0 О 1.0 O 7.0

A: Moles of HCl = 1.0 × 10-11 moles Volume of water = 1.0 Liter

Q: The pain reliever codeine is a weak base with a K, equal to 1.6x10-6. What is the pH of a 0.05 M…

A: pH of a solution is defined as the negative  logarithm of H+ ion concentration. Given codeine…

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.