10 -- 56 89 2 3 : : Question 4 Listen 01.3x10-6 M Listen Find the [OH-]in a solution where [H30*]=7.7x10-9 M 01.0x10-14 M 01.3x107 M 07.7х10-5 м Find the (OH Jin a solution where [H30*]=5.6x10-6 M 01.8x109 M 01.0x10-14 M 05.6x10-6 M 01.8x10-10 M

Q: OH OH OH OH ČH3 'N' `CH3 Br H' CH3

A:

Q: HSO4-(aq)+ H2O(l) H2SO4(aq)+ OH-aq   the base is  OH- HSO4- none H20 H2SO4

A: According to Bronsted Lowry theory, Acid is species which donates  proton and base is species which…

Q: What is the [OH-] in a solution that has a [ H3O+]- 1 × 10° M? A) 1× 102 M B) 1 × 10 M C) 1 × 108 M…

A: The concentration of hydronium ion,The concentration of hydroxide ion = ?

Q: 44. In the equation below; C6H5NH₂(aq) + H₂O(l) ⇒ CH₂NH₂ (aq) + OH¯(aq) Which compound is considered…

A: Conjugated acid and conjugate base:

Q: Name: NetID: 18. What is the pOH of a 0.18 M benzoic acid (C6H5COOH), at 25 °C, if the K₂ of the…

A:

Q: Write an equation for the reaction in which H₂C8H7Os (ag) acts as a base in H₂O(1). Express your…

A: Acid base reaction gives the salt and H2O as a product. So following type of reaction observed:-

Q: A weak acid has a Ka = 5.78x10. What is its pK3? %3D 9.244 8.238 O 1.660 0.999

A: Given, the Ka for a weak acid = 5.78 × 10-9 We have to calculate the pKa of the acid.

Q: 1. What is the pH of a solution with [H 3O +] = 1 × 10 -1 M

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: In which of the following aqueous solutions does the weak acid exhibit the highest percentage…

A: For acidic solution, [H3O+] > [OH-] For basic solution, [OH-] > [H3O+]     According to…

Q: If [H* ] = 4.3 x 10-4 M, what is [OH]?

A: The given problem can be solved by using the formula given below as; H+ OH- = Kw= 1.0×10-14…

Q: Calculate the [H30+]value of{OH-}=1.2x10-11M

A: We have to calculate the [H3O+]

Q: Strong acids HCI HBr HI HCIO4 HNO3 H₂SO4 Weak acids HF HNO2 NH3 HCN HCOOH CH3COOH Previous Answers…

A: Acid : Acid are those substancesWhich can donate H+ ion Whicn can accept lone pair of electronAll…

Q: solution with [OH-1] = 5,4 x 10-6 has [H+]=?   a. 1.8 x 10-9   b. 1.9 x 10-9    c. 5,4 x 10-20…

A: The relationship between OH- and  H+ is as follows: OH-H+=Kw where Kw is the ionic product of water…

Q: In an aqueous solution at 25°C, if [H,0*] = 3.5 x 10-4 M, then [OH-] is:

A: Provided concentration of [H3O+]=3.5×10-4 M Product of concentration of H3O+ and OH- is equal to…

Q: The first question/screenshot is the beginning structure, but I don't need help on that anymore. It…

A: Concept based on the organic chemical reactions and their mechanisms. Each and every step in the…

Q: -log [H+] -log[OH-] alog (-pH) alog (-pOH) Soln pH рон [H+] [OH-] A 3.2 В 1.9 2. 5 E -10 D 1.6 E -3

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Q: Decide which compound is the acid and which is the base, and draw the products of the proton…

A: Answer:- acids are the proton donor and the bases are proton donor. The species formed after the…

Q: Question 11 Calculate the [OH-] in a solution with [H*] = 7.9 x 10-5 %3D Hint: Water constant: Kw=…

A: Given [H+] = 7.9*10-5 Kw = 1*10-14

Q: SAMPLE Calamansi Tap water Distilled Water Vinegar Sugar in water Baking soda Comstarch Soft drink…

A: Acid or Base  Depending on how one chooses to see the characteristics of acidity and basicity, the…

Q: Which would you predict to be the weakest acid?    Lactic Acid (Ka = 1.4 x 10-4)        Hydrofluoric…

A: Acidity: The acidic nature of chemical substances can be determined by their pH value. Stronger acid…

Q: What are [H*] and the [OH-] in a 0.10 solution of a weak acid ? Ka=1.0 x10-7 1.0 x10-6 and 1.0 x…

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Q: Which of the following is expected to be the strongest acid? Choices: H2SO3…

A: Acids which have higher value of ka is Stronger Acid. As from given Ka values, H2CO3 has higher Ka…

Q: Which of the following is a strong acid? O acetic acid Ohydrochloric acid hydrofluoric acid…

A: The strong acid among them is given below

Q: What is the [OH-] in a solution with [H₂O+] = 6.38 × 10-¹¹ M? A B с D E 1.75 x 10-7 M 1.5 × 10-12 M…

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Q: [H+] = 4.8E-3

A: Applying formula of pH  PH = -log [H+]

Q: What is the [H 30 *] in a solution with [OH-] = 1 × 10-12 N -M?

A:

Q: 13. Circle the molecule that is the weakest Bronsted acid: H2O, CH4, HF, HCl, NH3

A: According to the Bronsted's theory of acid and bases, any molecule that donates proton is an acid…

Q: Use the Ka values for the following acids to find the strongest conjugate base: HSO4- 1.2 x 10-2…

A:

Q: What is the H+ of a solution with [OH-] =  6.22 x10-11 M at 25 oC? Group of answer choices 1.61 x…

A: Given datas ;  At 25°C  [OH–] = 6.22 × 10-11 M  [H+] = ?

Q: Match each solution with the correct description…

A: Given: To match the following: 1. dilute weak acid  18 M sulfuric acid 2. dilute strong base…

Q: What are the products in the reaction: HCO31+H20 if the H20 is acting as a base? H2CO3+H2O O…

A: Here, we have to find the products in the reaction: HCO3-1 + H2O when H2O is acting as a base.

Q: Which H atom in vitamin C (ascorbic acid) is most acidic? Select the single best answer. P OH-b НО O…

A: The acidity of an organic molecule (AH) depends on the following factors:A-H bond strengthStability…

Q: 13 1 point Consider the reaction HC204 HNO2 --> NO2 H2C204 Which species is the conjugate acid?…

A: Acid : It is a substance that contains Hydrogen and can donate it to other molecules or substances.…

Q: Original acid HNO3 H₂O H₂O + HBr HCO3- Original acid HNO3 H₂O H₂O + HBr HCO3 Conjugate base…

A: Conjugate base obtained from removal of H+ from the original acid. Thus,

Q: [OH] = 3.3E-1

A: Answer given as follows

Q: Modify the three molecules so that they show the form that is dominant at physiological pH :   Since…

A:

Q: 6. N-H + Kolt ~NH₂

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: Draw and label a representation of a concentrated solution of a weak acid: T-3 Draw and label a…

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Q: Construct the expression for Kc for the following reaction. H,O(1) = H*(aq) + OH-(aq) Drag the tiles…

A: Given H₂O(l) ⇌ H+ (aq) + OH- (aq)

Q: Using the equilibrium below, select the statement consistent with favorability NH NH2 NH3 NH2…

A: Given : We have to tell which statement is correct.

Q: What is [OH-] in a solution with [H+] = 9.78x10-9 M? a. 1.02x10-10 M b. 1.0x10-24 M c. 9.78x10-23 M…

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Q: Determine whether the acid is mono-, di-, or tri-protic. HO₂CCH₂(COHCO₂H)CH₂CO₂H O monoprotic…

A:

Q: Question 5 Which one of the following statements is true? H pka - 10 O NH₂ H Question 6 NH₂ pka ~35…

A: We know K = [ product] / [reactant]

Q: Consider these potential pharmaceutical drugs (where the symbol R is used to represent the rest of…

A: The acidity of the compound is related to the ease by which the H atoms are removed as H+ from the…

Q: 8. The acids in Table 2 are divided into two groups: those with Ka > 1 and those with Ka < 1.…

A: In the given table, the acids are divided into two groupsi) The group that has Ka value greater than…

Q: None

A: The concentration of hydronium ion  = [H3O+] = 6.61×10-2M [OH-] = .....M To calculate the hydroxide…

Q: Given the following data:   Base                      Kb   NaF                       1.47  x…

A: Which of the following is the strongest acid? HF HC6H5O HClO H2SO3 HC2H3O2

Q: [H+] = 6.5E-12

A:

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.