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

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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 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: 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…

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

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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: 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.