Calculate [OH-] if [H3O+]=4.01x10^-4 and [H3O+]=7.22x10^-6

Q: identify the role of water ( acid, base, or neutral )

A: According to Bronsted-Lowry concept,an acid releases an H+ ion to become conjugate base and base…

Q: find the pH and [OH-] if [H3O] = 7.8 x 10^-8

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Q: Consider the following data on some weak acids and weak bases: acid base K. K, name formula name…

A: pH = -log[H+] HA  =   A-  +  H+   K is equilibrium constant K = [A-][H+]/[HA] pKa = -log Ka So,…

Q: Calculate the pH for the following concentration: [H3O+] = 2.19 x 10-5 M.

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Q: Give the formula of the conjugate acid:(a) NH₃(b) NH₂⁻(c) nicotine, C₁₀H₁₄N₂

A: The species which accepts a proton in the bronsted acid base theory. The species which accepts a…

Q: Is the self ionization of water endothermic or exothermic? The ionization constant for water (Kw) is…

A: The self ionization reaction of water is  H2O (l) ---------> H+ (aq) + OH- (aq) The ionization…

Q: write the chemical formula of the base: Cl-(aq)+HSO4-(aq)  HCI(aq)+S042-(aq)

A: The given reaction is shown below.

Q: conjugate base formula HS 1.8 x 10

A: Using , Ka × Kb = Kw Kw = 1 × 10-14

Q: calculate [OH-] IF [H3O+] = 4.01 X 10 -4 AND [H3O+] = 7.22 X 10 -6

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Q: 2. Calculate the [OH-] of water at SATP if the hydrogen ion concentration is 0.2 mol/L.

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Q: 6. Convert the following pH or pOH values to [H*] or [OH] concentration Example: pH = 7.0, [H*] =…

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Q: Which of the following shows the ionization of hydrochloric acid in water? A H30* + CI HCI + H20 В…

A: The correct equation that represents ionization of hydrochloric acid in water.

Q: If the pH of a solution is 3.9, calculate [H*]. O 0.011220185 O 89.125093813 O 7943.282347243 O…

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Q: Calculate the pH for the following concentration: [H3O+] = 3.24 x 10-3 M

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Q: Show complete calculations Calculate the pOH, H3O+, OH- if the pH is: 1. pH = 8.3 2. pH = 14

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Q: How much more OH- is in water at a pH of 11 when compared to pH of 7?

A: Step 1-In this question we have to compare the OH-concentration in water at pH = 11 and at pH = 7.

Q: [H30] [OH] pH Classification (acid, base or neutral) 4.8 x 104 6.5 x 10 2 7.0 9.5 x 10-9

A: To fill the given table by using given data

Q: Acid, base or neutral [H*] [OH'] pH pOH 3.25 х 106 М 4.5 9.5 2.7 11.3

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: 1. Convert 8.62  pH value to OH- concentration (in mM).

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Q: If a sample of a certain solution is determined to have a [H3O+] concentration of 8.94×10^−4…

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Q: Calculate [OH-] given [H3O+] = 4.0 * 10^-9 M

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: What pH most likely corresponds to the following expression: [H+]=[OH-] O pH 5 O pH 6 O pH 4

A: We know that pH = 7 means the neutral solution That means concentration of [H+] are equal to…

Q: 4. Complete the table below and answer the questions. For the Column 4, multiply [H+] and [OH-]…

A: pH is equal to the negative log of the hydronium ion concentration. pOH is equal to the negative log…

Q: Write the conjugate base formulas of the following base: а. HF b. HNO3 c. HSO3

A: Conjugate base is formed after when an acid loses its proton.

Q: Use the following information to complete the statement below. Solution Information Provided 1 2 3 4…

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Q: Arrange the acids in increasing order of acidity. highest. To rank items as equivalent, overlap…

A: Acidity order of different substances can be identified by comparing their pH values. A pH value…

Q: Kw of water at 100°C is 5.62 x 10-13. What is the pH of water at this temperature

A: Given- Kw = 5.62 × 10-13 T= 100°C = 100 + 273 = 373 K

Q: If the pH of a solution is 6.8, calculate [H*]. O 2511.886431510 O 0.000398107 O 0.000000158 O…

A: Relation between pH and H+  pH = -log[H+]  We want to determine [H+] concentration  -pH = log[H+]…

Q: find [OH-] and [H3O+] if the pH= 2.75

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Q: Write equations that show H2 PO4− acting both as an acid and as a base.

A: An acid is a substance that can donate a proton. Conjugate base is formed when an acid has donated a…

Q: Show complete calculations Calculate the pOH, H3O+, OH- if the pH is: 1. pH = 8 2. pH = 7.4

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Q: Conside following data on some weak acids and weak bases: acid base K, a name formula name formula…

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Q: 5. Identify each of the following as an acid or a base. HCI NaOH H2SO4 NaNH2 K2CO3

A: 5.  An acid is a species which can donate a proton ( H+ ) or an electron acceptor and base is a…

Q: Rank the following solutions according to their acidity: Rank Solution 1 H30+ = 1012 M [H,O*…

A: The acidity of a solution is described by the pH scale. pH is the measurement of the hydronium ion…

Q: 2. In the equation depicting the autoionization of water, H20 H+ OH- The reaction proceeds far to…

A: This reaction occurs between 2 molecules of water which ionise in hydronium ion and hydroxy ion .…

Q: Q1 Complete the following table: [H3O*] [OH"] Acidic, Basic, or Neutral? pH 2.0x10-6 9.8 3.5x10-3 01…

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

Q: When the concentration of H3O+ and OH- ions are equal in a cup of water, the water's pH will be a.…

A: Th number of H3O+ and OH- ions in the cup of water are equal.

Q: Identify the following species:  KClO HHlO4 NH4Cl H2SO4 The choices to pick from for each are as…

A: An acid is a substance which has the tendency to furnish H+ ions in the aqueous solutions. For…

Q: Determine the pH of a solution with an [OH-] = 3.6 x 10-10 M.

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: List the following by ability to ionize, least to greatest. (#1 being the greatest and #5 being the…

A: Ka refers to the acid dissociation constant. It is said that the higher the Ka, the more possibility…

Q: For numbers 1 to 3, determine if the given condition is (A) acidic, (B) basic, (C) neutral. or (D)…

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Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: Given that : We have to rank the following solutions in order of increasing pH :

Q: Select the two Bronsted acids from the following list HCN NH4+ OH NO2+

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Q: pOH = 10.85 What is the acid AND the base. (I need both)

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Q: 4) Complete the following table. Show all your work including formulas. [H'] M [OH]M pH pOH Acidic,…

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Q: H,N-ÇH-COO CH2 a. neutral, nonpolar b. basic, polar c. neutral, polar d. acidic, polar

A: b) basic, polar

Q: If the pH of a solution is 9.7, calculate [H*]. O 70794.578438414 O 5011872336.272714615 O…

A: pH = - Log[H+] [H+]= -antilog[pH] [H+]= antilog[-9.7] [H+] = 1.99 * 10-10

Q: Show complete calculations Calculate the pOH, H3O+, OH- if the pH is: 1. pH = 7

A: The question is based on the concept of PH and pOH calculations. pH is defined as negative…

Q: List the following by ability to ionize, least to greatest. HC7H5O2, Ka = 6.3x10-5 HC2H3O2, Ka =…

A: The higher the value of Ka, the higher will be the value of ions produced. Thus, the value of Ka is…

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: Solution                0.1 M C6H5NH3Cl      0.1 M KCl                     0.1 M KClO…

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.