Calculate the pH of 5.85 E-4 M solution of magnesium hydroxide. (Ans= 11.068) not sure how my teacher got that answer, so plz show work. Thanks in advance

Q: 3empis left Check my work Be sure to answer all parts. Be sure to reportyour answer to the correct…

A: Given that, Ka value of conjugate acid HB+ of weak base HB = 8.3×10-4 Kb value of weak base HB = to…

Q: O Other Boc (EOC) [References] Consider 45.0 mL of a solution of weak acid HA (K water must be added…

A: Here 45 ml of weak acid HA (ka= 1.4×10^--6) has pH 4.25 is diluted and the pH becomes 5.25 . We have…

Q: 9. If only 1.6% of 0.20 M solution of a weak base was ionized. Calculate its Kb value? *

A:

Q: Determine the pH of a 0.31 M solution of NaN3 (Ka for HN3 = 1.9 × 10−5). Express your answer using…

A: NaN3 is salt of weak acid and strong base and it is basic salt  pH = 1/2 ( 14 + pka + log C)

Q: Using the Kb from the previous question, what is the pH of an 0.0100 M solution of sodium benzoate.…

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Q: The pH of 0.17 M of HCN is Ka of HCN = 1.6 x 10 10 %3D (Write your answer to 2 d.p. eg: 7.65)

A: The question is based on the concept of chemical equilibrium. we have been given a weak acid…

Q: Calculate Kh using the equations, whichever is applicable. (If the ion is conjugate acid of a weak…

A:

Q: SHOW WORK. Perform the following calculations & determinations for this solution. 6.84 x 10-2 M OH…

A:

Q: 1.80

A: Dear student I have given answer to your question in the image format.

Q: Determine whether the following salts are acidic, basic, or neutral. Explain your answer. а. KS b.…

A:

Q: What is the pH of a 0.391 M HNO3 solution? Your Answer:

A: Given data  The concentration of aqueous HNO3  solution = 0.391 M, The pH of a 0.391 M HNO3…

Q: The pH of 0.1 Mof HCN is Ka of HCN = 1.6 x 10 10 (Write your answer to 2 d.p. eg: 7.65) Answer:

A: Given information,    Concentration of HCN = 0.1 M    Ka for HCN = 1.6 x 10-10

Q: Show all steps: What is the percent ionization of a 1.38 mol/L weak base if its Kb = 2.7 x 10-6?

A: Given, concentration of weak base = 1.38 mol/L = 1.38 M  Kb, = 2.7 x 10-6  % Ionization = ?

Q: Acids & Bases: Understanding Connections Between Descriptions if Weak Acid Dissociations For a…

A: First, the acid dissociation constant, Ka for given acid is calculated as follows,

Q: Determine the pH  and the concentration of [OH– ] in a 0.40 M solution of ammonia?       The Kb…

A:

Q: The pH of an aqueous solution at 25°C was found to be 3.90. The pOH of this solution is The…

A: pH is defined as the negative logarithm of hydrogen or hydronium ion concentration present in the…

Q: The base protonation constant K, of azetidine (C;H,NH) is 1.5 × 10-8. Calculate the pH of a 0.31 M…

A: The pH of the solution can be determined by using ICE table and equilbrium expression for the given…

Q: What is the pH of a 0.03 M weak acid solution? The K, of the said acid is 5.0 x 10. Note: Do not use…

A: Given :-  Concentration of weak acid = 0.03 M  Ka of acid = 5.0 × 10-5  To calculate :-  pH of…

Q: The K, for hydrofluoric acid HF is 6.8 x 104. (4 points) Calculate K, for its conjugate base F…

A:

Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kb of NH= 1.8 x 105) NH4* + H2O+…

A: In the given question we have to calculate the pH of 0.6 M NH4Cl Solution. we know that the ammonium…

Q: www y wun LU you U I M v o reference (Page) section 16.3 while problem. CIO, accepts a proton from…

A: To draw a formula large atom should be in central and more electronegative atom should be something

Q: (Q19) What is the pH of a solution that is 0.768 in hydrosulfuric acid (H2S)? Ka1 = 8.9 x 10-8 and…

A:

Q: What is the pH of a 1 x 10-5 M NAOH solution? Your Answer:

A: pH is defined as " The negative logarithm to the base 10 of concentration of H+ ions expressed in…

Q: (Q19) What is the pH of a solution that is 0.720 in hydrosulfuric acid (H2S)? Ka1 = 8.9 x 10-8 and…

A: PH of H2S can be calculated as follows

Q: Important equations: Ka × Kb = KwpKa= −logKa   A key component of understanding weak acids is…

A: HBr ,HCl,HI etc are strong acid so dissociation constants will be very high.

Q: 11 5, de /188795/assignments/3601808 Homework Ch16 - Attempt 1 Problem 16.61 3 of 15 Constants |…

A: Given- Concentration = 0.13M pKa = 2.32

Q: What is the pH of a 0.039 M HNO3 solution? Your Answer: Answer

A: In this question, we want to determine the the pH of HNO3 Solution.  How we can determine, you can…

Q: Which compounds are Lewis acids? Select all that apply. (CH3)3C* BeCl, Br CH;CH,OH

A: According to lewis concept, the substances that accept electron pairs are called lewis acids. And…

Q: Calculate the pH of a 5.3 M solution of alloxanic acid. Round your answer to 1 decimal place.

A:

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: yo 1. The pH of Coca-Cola is 2.52. How many moles of H* is present in 1.0 L of Coca-Cola? Show:…

A: Use formula of pH and get the answer

Q: 1. Place the following 0.10 M solutions (aq., 25 oC) in order of increasing pH: Format: R < S < T <…

A: pH= -log[H+], and for weak acid the it will not dissociate completely, so [H+]= (c.Ka)½ Where Ka is…

Q: What is the pH of a 0.306 M HNO3 solution? Your Answer:

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: What is the pH of a 0.0515 M NaOH solution? Your Answer:

A: Given [ NaOH]=[OH]=0.0515 we have to find pOH

Q: Find the Ka of a weak acid ( HA ) that has a concentration of 0.020 M. The pH is 2.74.

A: Weak acid  [H+] and Ka are related as  [H+] = ( Ka x C)1/2 Where C = concentration of acid = 0.02…

Q: List the following bases in order of strength, strongest to weakest. O NH4OH, Kb=1.8x10-3 O NH3,…

A:

Q: Show work for (a) on answer sheet.   If needed:   Kw = [H3O+] [-OH] = 1.00 x 10 -14  M…

A:

Q: Would you help me whit this example (1) Thank you.   ın a solutıon with a pH value of 7.0, Find…

A: Given : PH of solution = 7 Ka value of HOCl =3×10^-8 To find : percentage dissociation  Solution :…

Q: What is the expected pH of a 150.0 mL 0.250 M solution of HOCI which is diluted to a 500.0 ml mark…

A: Given that, a 150.0 mL of 0.250 M solution of HOCl is diluted to 500.0 mL, i.e., V1 = 150.0 mL, S1 =…

Q: -5 Calculate the pH of a 5.7 × 10 °M aqueous solution of hydroiodic acid (HI). Round your answer to…

A: Since HI is a strong acid  hence it will dissociate completely as per the reaction  HI -----&gt; H+…

Q: Is the response below correct, I would belive that   pOH = – log (12.7) = 1.103 would be -1.103…

A: Since U asked about the calculation and Answer check. See the correct Solution below.

Q: 1. The formula for the conjugate base of H₂S is 2. The formula for the conjugate acid of HC6H606 is…

A:

Q: A 0.25 M solution of a weak acid has a measured pH = 2.55. On a separate piece of paper, determine…

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

Q: If the Kb value for a weak base is 2.6*10^-4, what is the value of its conjugate acid?

A:

Q: QUESTION 11 (4c-401) Which of the following solutions is most basic? Show all work to support your…

A: Basic solutions are those which have pH values of more than 7. Higher is the pH value more it will…

Q: 16.72

A: The given balanced chemical equation – The given concentration of BrO- = 0.724 M And the Kb = 4.0 x…

Q: Determine the OH, pH, and pOH of a solution with a [H*] of 3.8 x 10-5 M at 25 °C. [_HO] pH %3D pOH =

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

Q: What is the [H3O+] of 0.10 M propanoic acid (CH3CH2COOH, can simplify to HPr) (Ka= 1.3x10−5)?…

A: pH of a solution measures acidity of the solution.  pH + pOH = 14 Where, pH = -log [H3 O+ ] and pOH…

Q: In each row, check the box under the compound that can reasonably be expected to be more acidic in…

A:

Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kb of NH= 1.8 x 10) NH4* + H2O+→…

A: Ammonium chloride is a salt, so it water it will donate proton to water and form ammonia and…

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.