5. Refer to the figure to answer the questions a & b. a. What is the pKa of the unknown acid? _______________ b. What is the Ka of the unknown acid?

Q: What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NHẠCH (Pkb of NH3=4.75) O 2.15 4.62…

A: Given:- NH3 = 0.20M = BaseNH4Cl = 0.15M = Saltpkb of NH3 =4.75pH = ?

Q: 2. Oxalic acid (a diprotic acid HOOCCOOH; pKal 1.25 and pKa2 = 4.28 at 25°C) is added to pure water…

A: The objective of the question is to determine the final pH of a solution of oxalic acid in water and…

Q: The effectiveness of a buffer depends on all of the following except ___________.   A the absolute…

A: Here we have to determine the statements from the following which are not effective for a buffer…

Q: a) What is the {H*} activity if the pH measured in the lab with a pH meter is 12 (in DecExp)? (5…

A:

Q: A ONLY A solution is prepared that contains 0.2 M NaBrO2 (Kb BrO2- =8.3x10-10) and 0.1 M NH3 (Kb…

A: We have two weak bases in the solution,  Between these two weak bases, the Kb value of BrO2- is very…

Q: C i Curved arrows are used to illustrate the flow of electrons. Using the provided starting…

A:

Q: 8.29) For each of the following conjugate pairs, predict whether the acid form or the base form is…

A: Answer: Any acid-base conjugate pairs when pH is less than pKa then acid form predominate over base…

Q: a. Which combination of acid and salt will make a good buffer solution? i.HNO3 and NaNO3 ii. H2CO3…

A: Buffer Solutions are the solutions which resists the sharp change in pH on addition of an acid or…

Q: An acetic acid solution contains both acetic acid (conjugated acid) and acetate ions (conjugated…

A: Given data:Calculate the ratio, mole fraction and concentrations of acetic acid and acetate.

Q: Calculate the pH at 25 "C of a 0.35M solution of potassium butanoate (KC,H,co.). Note that butanoic…

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Q: True or false (7).  The greater the Ka value,   the more dissociation the weak acid.___________…

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Q: For the second dissociation of H, CO3: HCO3(aq) + H,O=H;O) + COaq) + CO3(aq) (1) a. At what volume…

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

Q: I know the correct answer, I just don't how to get to the answer

A: To determine the pH of a saturated solution of magnesium hydroxide, we need to consider the…

Q: Unit 20 3. The carbonate buffer system is very important in regulating blood pH levels. Carbonic…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: can you help me calculate the percent error for my pKa? my pKa = 6.79 my Ka = 1.62 x 10^-7 the…

A: The experimental value of pKa of NaHSO3 = 6.79 NaHSO3 is a single deprotonated form of H2SO3 whose…

Q: QUESTION 11 If the pKa of HCHO2 is 3.74 and the pH of an HCHO2 /NaCHO2 buffer solution is 3.74,…

A: The given information is as follows:        The pKa of HCHO2 = 3.74The pH of the  solution = 3.74The…

Q: Fast pls i will give u like for sure pls solve in 2 min pls answer the following: 1) Calculate the…

A: 1) concentration of HF = 0.15 mol/lt Ka = 6.6 x 10-4…

Q: Activity 4. It's Solving Time! Directions: Solve the following problem. Write your complete…

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Q: Macmillan Learning What are the concentrations of H₂O+ and OH in oranges that have a pH of 3.82?…

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Q: 02. A 10.00 mL sample of phosphoric acid was titrated to endpoint with a 0.2222 M NaOH solution. The…

A: Phosphoric acid reacts with sodium hydroxide to form sodium phosphate and water. The equation for…

Q: Which of the following rows identifies the common classification of C₂H4(g) and C₂H4Cl₂(g), and…

A: Answer  of ist question is first line of the table: aliphatic| unsaturated| saturated

Q: Calculate the volume of 0.650-M NaOH solution needed to completely neutralize 28.1 mL of a 0.760-M…

A: The neutralisation reaction taking place will be  2 NaOH + H2SO4 --------> Na2SO4 + 2 H2O hence…

Q: If the Ką of a weak acid is 1.6 x 10-8, the Kp of its conjugate base must be which of the following?…

A: There is the relation between the Ka (acid dissociation constant) and  Kb (base dissociation…

Q: 5.796

A: Kb = 10-pKb  Kb = 10-5.796 Kb = 1.6 • 10^-6

Q: What I Have Learned Activity 3.6: Calculate the following concentration. 1. What is the…

A:

Q: What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M…

A: We would use Henderson Hasselbalch equation to calculate the concentration of acetate.

Q: 3.1). The following plot represents the potentiometric curve of acid with NaOH. Volume of NaOHL m a)…

A: Step 1: From the graph, the equivalence point is 22 mL.The volume of NaOH at which there is a steep…

Q: If the pH of 1 liter carbonate buffer is 7.0, what is H₂CO3 and HCO3? (pK₂ = 6.37) What component is…

A: When dealing with a carbonate buffer with a given pH of 7.0 and a pK₁ value of 6.37, we can use the…

Q: The difference in the concentration of hydronium ions in a solution of pH 2.0 compared with one of…

A: We know that : pH = -log[H3O^+]  [H3O^+] = concentration of hydronium ion.  For pH = 2 :  2 =…

Q: 16.At the midpoint of a titration curve for valine A. The concentration of a conjugate base is equal…

A: At the midpoint of a titration curve for valine:A. The concentration of a conjugate base is equal to…

Q: Determine the Ka of each solution  Sol. A – 20 mL of 1.00 NaA and 10 mL of 1.00 M HA Sol. B – 20…

A: Acidic buffer and use of Henderson hasselbalch equation for pH calculation:

Q: 2. Calculate Ko for OBr from pH of a 0.10 M solution of NaOBr. the equation for th

A:

Q: Which of the following is an amphoteric species? Select one: a. LiOH b. None of these c. HSO4- d.…

A: 1.we know that amphoteric compounds are a chemical substance that might be a neutral molecule or an…

Q: 9.Circle the pH value for each of the following 0.1 M solutions: a. NH,CI 1 between 1&7 between 7&13…

A: Given : Concentration of salts are 0.1 M. pH of any salt solution is decided by the nature of the…

Q: A solution is made by dissolving 33.5 g of Ba(NO₂)2 in 500.0 mL of water. Using Kb(NO₂) = 2.2 ×…

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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.