The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

Q: Seawater has a pH of 8.10. What is its hydrogen ion concentration? 1.0 x 10-8 8.0 x 10-1 7.9 x 10-9…

A: We know that pH = -log[H+] So [H+] =10^-pH

Q: ⁻ concentration in an aqueous solution at 25 °C is 1.1 × 10⁻³. What is [H⁺]?

A: Product of hydrogen ion concentration and hydroxide ion concentration is equal to ionic product of…

Q: Part A Water ionizes by the equation H2O(1) =H (ag) + OH (ag) The extent of the reaction is small in…

A: We have given poH and have to find [H+] in A part, rank in b part and kw in C part

Q: What is the pH of .08 M H2SO3 (aq)? O 12.51 Ο 1.10 0 .94 O 1.89 Ο 1.49

A: Concentration of H2SO3 = 0.08 M  pH of the H2SO3 = ?

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.3 × 10⁻⁵. What is [H⁺]?

A: Given: [OH- ] = 2.3 × 10-5 M

Q: Can hydroxide ion (OH-) exist in liquid sulfuric acid (H2SO4)?  If so, justify your answer.  If not,…

A: Acid base reaction are very fast.

Q: To answer this question, you may need access to the periodic table of elements, a calculator, and…

A: Here we have to calculate pOH of a 0.000259 M HClO4 solution at 25° C.

Q: Calculating the pH of a weak base solution The base protonation constant K, of morpholine (C,H,ONH)…

A:

Q: What is the pH of 4.3 x 10-4 M NaOH (aq)? O 17.4 10.6 О 3.4 O -3.4 O 24.6

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Q: what is the pH of a 0.40 M Solution of NH 4 NO3(aq)? Kb for NH ₂ (aq) = 1.76X10²5

A:

Q: What is the pH of 0.03 M HNO2?

A: Given :-  Molar concentration of HNO2 = 0.03 M  Ka = 4.6 × 10-4  To calculate :-  pH of the solution

Q: Determine the pOH of a 0.625 M HClO solution. Ka = 3.0 x 10-8

A:

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: What is the pH of .03 M NH4Br (aq)? O 3.13 O 9.25 O 10.87 O 1.52 O 5.38

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Q: Identify the acid and the base in each Lewis acid-base reaction. H2O + SO3 → H2SO4

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Q: What is the pH of 3.7 x 103 M NH¼Br(aq)? Ο 10.4 O 2.4 Ο 11.7 O 5.8 O 4.6

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Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

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Q: 12 . What is the expected pH of a 0.015 M solution of boric acid (assuming 100% dissociation) ?

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Q: What is the pH of .15 M KBRO(aq)? O 3.07 O 4.75 O 13.18 O 9.25 O 10.93

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Q: What is the pH of a 0.193 M w. acid HA solution? Ka = 6.61 x 10−6?

A: The acid is weak so it weakly dissociates in the solution. That is it gives an H+ ions slowly in to…

Q: -2 Calculate the pH of a 1.0 x 10 M solution of HNO,. Round your answer to 2 decimal places. pH=…

A: pH = - log [ H+]Here given acid is monobasic i.e. HNO3Given :-[H+] = 1.0*10-2 M

Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: What is the pH of 7.8 x 105 M HNO3 (aq)? O 18.1 O 9.9 O 9.5 O 3.7 O 4.1

A:

Q: 4. HCO 3 +H O2 Acid: Base: CA: CB:

A: Acid is a substance that is able of donating a H+ ion. Base can abstract the proton from an acid.…

Q: What is the pH of .76 M CN (aq)? O 13.9 O 4.7 O 9.3 O 2.4

A: Interpretation : We have to calculate the pH of CN- .

Q: Hydrazine, N2H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K of…

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Q: Explain how ammonia can function both as a Brønsted base and as a Lewis base.

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: Which of the following statements is/are correct at 25 °C? 1. Benzoate (C,H;O2) requires a Ka to…

A: To determine pH we need Ka or Kb value. Which among Ka or Kb is used depends on the nature of…

Q: Calculate the pH of a 0.025 M solution of propanoic acid (K, = 1.3 x 10-5). 7.48 0.025 O 5.6 x 104…

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Q: Calculate the pOH of a solution that contains 3.9 x 10 mol L H,O* at 25 °C. O 10.59 O 3.31 O 9.14 O…

A: The hydrogen ion concentration of the given solution is = 3.9×10-4 mol L-1 The pOH of the solution…

Q: What is the pH of 6.3 x 10-4 M Ba(OH)2 (aq)? Ο 11.1 O 10.8 O 3.2 O 2.9 O 7.6

A: We have to calculate the pH of 0.00063M Ba(OH)2 solution.

Q: Determine the hydroxide ion concentration in an aqueous solution of HBr with pH = 3.98 at 25 °C.…

A: Given: pH= 3.98 As we know, pH= -log[H+] So, [H+]= 10-pH  [H+]= 10-3.98  [H+]= 1.04 ×10-4M…

Q: Calculate the pH of a solution with a H,O* concentration of: 1.5 x 10 6 M

A: The solution’s pH is equivalent to the negative of the log of H+concentration which is generally…

Q: What is the pH of a 3.00 x 10−8 M solution of HClO4? 6.48 7.00 6.89 7.52 7.15

A: Applying formula  pH = - log[H+] = -log[H3O+]  Equation  HClO4(aq) ———>  H+(aq)  +  ClO4-(aq)

Q: A 0.030 M aqueous solution of a sodium salt (NaA) has a pH of 8.23. What is the value of K, for the…

A: The correct answer is given below

Q: 10. Calculate the pH of a 0.250 M solution The Ka of HCIO is 2.9x10-8.

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Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are…

A: Since the volume and concentration of acid taken is same for all acids  Hence the moles of all acid…

Q: Which of the following pH values would indicate a basic solution? 04 0 7 O 10 O 3

A: The answer to the following question is given as:

Q: What is the pH of .242 M H2CO3 (aq)? O 6.38 О 3.50 O 10.50 O 4.12 O 5.47

A: pH is defined as negative log of concentration of H+ ions in the solution.

Q: Of the following liquids, which one contains the lowest concentration of H3O+ ions? O Lemon juice…

A: pH : pH can be defined as the negative logarithm of hydrogen ion concentration pH = -log[H3O+] when…

Q: The pOH of a 0.07 M NgOH solution at 25 °C is:

A: Given :- concentration of NaOH = 0.07 M  To calculate :- pOH of the solution

Q: Calculate the pH at 25 °C of a 0.86M solution of potassium acetate (KCH3CO₂). Note that acetic acid…

A: It is based on the concept of hydrolysis of salt.Here we are required to find the pH of the…

Q: A 0.75 M solution of a certain weak base has a pH of 11.60. What is the K, for this weak base? O 3.6…

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Q: Calculate the pOH of the following solutions at 25 degrees Celsius. 1 [H+] = 1.0 x 10^-7 M* 2 [H+]…

A: First of all we know that relation between pH and pOH is :         pH + pOH = 14  Or.     pOH = 14 -…

Q: Draw a picture to represent the molecular view of the dissociation of HNO3 in water.

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Q: An aqueous solution has a pH = 4.23; what is the [ H3O+ ]? 5.9 x 10-5 M 17,000 M 1.7 M 5.9 x…

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Q: What is the pH of 2.7 x 102 M NaOH(aq)? O 3.6 O 1.6 Ο 12.4 O 13.1 O 10.4

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.