Q1\ Complete the following equations? -COOH + C,H3OH NII,OH он Ph Ph

Q: [OH-] = 4.2 x 10-2 Express the concentration to two significant figures and include the appropriate…

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Q: Calculate [OH-] when given the [H3O+] in each of the following aqueous solutions and classify the…

A: The OH- has to be calculated for the given aqueous solutions and whether they were acidic, basic or…

Q: A solution has a [H3O+] of 0.0015 M. Calculate the [OH-], the pH, and the pOH of the solution. Is…

A: In the question is given that concentration of [H3O]+  is 0.0015. i.e. [H]+ = 0.0015 [OH]- = ? pH =…

Q: Which of the following weak acids listed below is the strongest acid?  HF,HOCN,HC2H3O2,HOCl

A:

Q: iven the following: [H3O+] = 6.330 x 10-5,  calculate the pH:  (note: for pH always please use 3 sig…

A: pH = - log[H3O+] = - log(6.330×10-5) =5-log(6.330) = 4.20

Q: -HO + HOODHƆ ← 02 +0³H

A: Acids are proton donors and bases are proton-acceptors. An acid has a conjugate base which is formed…

Q: Write formula for the conjugate acid of the foll F O H2F O HF O H+ O 2HF

A: Conjugate acid of F-  ?

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

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Q: Indicate, by letter, the strongest acid and the weakest acid of those below. CH₂ a COOH (CH₂)₂N- b…

A: The objective of this question is to show the strongest and weakest acid. The substitutent attached…

Q: Calculate the concentration of H+ and OH- at 25°C. Say if the conditions are acidic, neutral og…

A: Recall the following relation to calculate H+  and OH- for the values of pH and pOH…

Q: If H+ is equal to 6.9x10^-5, what are the values of pH, POH, and OH-?

A: Given - [H+ ] =6.9*10-5 We have to determine pH, pOH and concentration of OH-.

Q: Identify the relative pH effect of KNO3. Group of answer choices Weak base Strong base Strong acid…

A: The question is based on the concept of salt hydrolysis. we need to identify the nature of salt and…

Q: For NH4Cl, predict whether the aqueous solution is acidic, basic or neutral and why. acidic because…

A: Given, The compound :   NH4Cl

Q: All of the following are weak acids except O HNO2 O HCN HBr НCNO HF

A: • we need to predict the strong acid from the given acids - HNO2 (Nitrous acid), HCN (Hydrocyanic…

Q: Give detailed Solution with explanation needed (no need Handwritten answer

A: A question based on reaction intermediate in organic chemistry. Structures of three organic…

Q: Given that Kw for water is 2.4 × 10-¹4 M² at 37 °C, calculate the pH of a neutral aqueous solution…

A: pH of solution is defined as negative logarithm of hydrogen ions present in solution.

Q: Given a solution in which the pH = 4, determine [H+], [OH-] and pOH.

A: Inorganic chemistry.

Q: g) H3P h) КОН

A: H3P=  pka value of PH3 is 27. It means that, pka value is more, so this is weak acid.

Q: Let X represent a nonmetal. Which of the following equal molar aqueous acid solutions has the lowest…

A: The pH of an acid depends on the: 1) The amount of H+. 2) The rate at which H+ is releasing. Faster…

Q: Write the formula for the conjugate acids of the following BL Bases. HPO4-2 CH3NH2 OH- HCO3-

A: Write the formula for the conjugate acids of the following BL Bases.

Q: Calculate the pH of a solution with an H+concentration of 5.6 x 10 ^-6 M and state if the solution…

A: We are given : H+ concentration = [ H3O+ ]  = 5.6 × 10 -6 M

Q: In converting from the pH of a solution to the corresponding H3O+ concentration, the following…

A: The answer of the given question is given below

Q: Complete the following table by calculating the missing entries. In each case indicate whether the…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: how is HCl an acid according to Bronsted-Lowry theory; write the equation while showing which…

A: According to Bronsted-Lowry theory, an acid is a substance which releases H+ ions in the solution.…

Q: Calculate the concentration of H3O+ in a solution that contains 7.1 x 1o-5 M OH- at 25°C. Identify…

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Q: Why are we using OH to solve for pH when we can just use H3O+ from the equation HCN +H2O = (H3O+) +…

A: Given -: [NaCN] = 0.021 M  Ka of HCN = 4.9×10-10  Calculate pH of solution

Q: Select the strongest acid in aqueous solution. O HOB. O These acids all have the same strength in…

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Q: Adding an acid to water increase the H3O+ ion concentration and decreases the OH- ion concentration.…

A: The statement is true or false has to mentioned

Q: • Part B Determine the pH for H,0") - 5.4 x 10 " M solution. Express your answer using two decimal…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the pOH of the solution. Is the…

A: [OH–] = 8.4 x 10–11 M( Given ) So, pOH = – log [OH–]  = – log( 8.4 x 10–11 ) = 10.075 Now, As we…

Q: By definition, a base dissolves in water to make a solution that contains: O hydroxide ion O H30*…

A: Given : When base dissolve in water To find : Product

Q: Which of the following is a strong base?     NaOAc     HCl     NaOH     HOAc

A: The conjugate base formed by the stronger acid will be weaker. The conjugate base formed by weaker…

Q: с) HF d) HNO2

A: C) HF is a weak acid D) HNO2  is a weak acid Ka of HF and HNO2 are 6.6×10-4 and 7.2×10-4

Q: Calculate the pH of a solution that has a concentration of OH- equal to 5.92 x 10^ (- 9) M.  (Write…

A: The objective of this question is to calculate the pH of a solution given the concentration of…

Q: 0.52 M KOH [H+] [OH-] PH POH

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Q: The pH of a solution is (6.5x10^0). What is the [OH-]? Report your answer to 2 sig figs. Note: Your…

A: Given, pH of the solution = 6.5 × 100 = 6.5 Concentration of the OH- ion = [OH-] = ? The formula…

Q: Indicate, by letter, the strongest acid and the weakest acid of those below. COOH The strongest acid…

A: The acidity of an acid is determined by its ability to donate a proton (H+) in a chemical…

Q: A solution increases the OH^- ion concentration of another solution Does the property describe a…

A: Please move to 2 step to get answer of your question Thank u

Q: Identify both conjugate acid/base pairs in the following reactions. Indicate the acid and the base…

A: According to Bronsted-Lowry concept  Acid is a species which donates H+ ion and forms its conjugate…

Q: How would I the conjugate acid and the base including ions pair and electron

A: Conjugate acid is a species able to donate proton and formed by accepting a proton of a acid.…

Q: Part A pH = 8.77 Express your answer using two significant figures. Enter your answers numerically…

A: Part A  pH = 8.77  pH = -log[H3O+]  Log[H3O+] = -pH  [H3O+] = antilog(-pH) = antilog(-8.77)  [H3O+]…

Q: Ascorbic acid (vitamin C) is a diprotic acid, H₂C6H6O6. Calculate [H*], pH, and [C6H6062] in a 0.17…

A: Information of question

Q: Select the strongest acid in aqueous solution. These acids all have the same strength in aqueous…

A: Strongest acid in aqueous solution is given below.

Q: A solution is added to water, and the H4 concentration of the water increases. Does the property…

A:

Q: 0.254M HNO3 [H+] [OH-] Ph POH

A: Given: Concentration of HNO3 = 0.254 M

Q: H,CO, H,SO,

A: Strong acid - H2SO4 , HNO3 Weak acid - H2CO3 , HI , HF

Q: Use the equation of the dissociation of the weak acid and a Le Schatelier principle to answer the…

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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.