Vhat is the pOH of a solution with [H,O)=1x10-5M 9. 4 10

Q: 9. A solution with a pOH of 4.65 at 25°C has a pH of .

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Q: The [H3O+] in a solution with pOH of 0.253 is ____.

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Q: For a solution of 0.020 M lactic acid, HC3H5O2 (Ka = 8.4 × 10-4), calculate: [H+]= _______ M pH=…

A: For a weak acid ,HClO                     HC3 H5O2       ⇌      C3 H5O2 -       +      H+…

Q: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

A: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

Q: Consider the following solutions at 25C. dentity the major species present in each solution and…

A: Answer:- This question is answered by using the simple concept of calculation of pH of aqueous…

Q: A solution has a H3O*concentration of 1.3 x 10-4. What is the pOH of the solution at 25°C?

A: Given- [H3O+]= 1.3 x 10-4 To find - pOH   Formula- pH + pOH = 14 pH = -log [H3O+]

Q: What is the pOH of a solution at 25C with a hydronium concentration at 5x10^-4

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Q: A solution turns red litmus blue, its pH is likely to be(a) 1(b) 4(c) 5 (d) 10

A: An important concept of pH can be given as: Acids have a pH level below 7 Bases have a pH level…

Q: Which of the following species is amphoteric? O co,? O HF O NHA O HPO42 None of the above are…

A: Amphoteric species are those which can act as both Brønsted -Lowry acid and Brønsted -Lowry base.…

Q: culate the [OH-]of the solution with pH=10.50 3.2 x 10-10 1.05 x 10-10

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

Q: An aqueous solution at 25 °C has a OH concentration of 1. x 10 ´M. Calculate the H,O' concentra x10

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Q: Calculate the pOH in 0.3582 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2 =…

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Q: What is the [OH] in a solution with a pOH of 6.48? [OH ] = [ ? ] × 10') %3D

A: [OH-] represents the concentration of hydroxide ions (OH-) in the solution pOH is just the negative…

Q: Which of the following dissociates completely (100%) into hydrogen and anions in solution? ak O a)…

A: Strong electrolytes are those which dissociates completely i.e. 100% into its ions.  Acids are those…

Q: Q5: Calculate the M for Al:(SOi)s solution has 0.3 N and Bi (NO): has 0.2 M?

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Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

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Q: A solution with a pOH of 5.55 has an [OH–] of __________

A: We know,                            pOH = - log[OH-]                    Or, log[OH-] = - pOH…

Q: What is the pH and the pOH of a 0.0215 M HCIO3 solution at 80.0 °C? Kw 2.5 x 10-13 at 80.0 °C pH:…

A: Given: Kw=2.5×10-13 [HClO3]=0.0215 M To find: pH and pOH Formula: pH=-log10[H+] pH+pOH=14

Q: The [OH] in a 0.20M solution of NH4OH is: (Kb for NH4OH = 1.8 x 10-5) 3.6 x 10-6 M O 1.8 x 10-5 M…

A: Given: Initial concentration of NH4OH=0.20 M Kb of NH4OH = 1.8×10-5 Let x be the dissociated amount…

Q: What is the pOH of a solution that has [OH ]eg = 1.5E-4 M?

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Q: iv) What name is given to the solution formed when all the NaOH has reacted? Calculate the p" of the…

A: The question is based on the concept of titrations. we are adding acetic Acid to the sodium…

Q: Calculate the pOH in a solution that has [H+]= 4.7x10-8 M.

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Q: Why is [ H3O] = [OH]  =1×10^-2M not feasible in water? What would happen if we tried to make such a…

A: The dissociation of ionisation reaction of water is  2 H2O (l) --------> H3O+ (aq) + OH- (aq)…

Q: Vhat is the pOH of a 0.0250 M HI solution? А. 0.944 В. 12.398 С. 1.602

A: Given : Molarity of HI = 0.0250M

Q: What is the pOH of the solution if the H3O + concentration is 4.5 x 10-4

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Q: Calculate the pOH of a solution with [OH-] = 6.8 x 10-9 M

A: Given  ; [OH-] = 6.8 × 10-9 M  To calculate the pOH of the solution.

Q: 12) Calculate the [H*], pH, and pOH for a 100.00mL of 0.00250M HCl at 25°C. [H*] = pH = pOH = _M %3D

A: Introduction: An acid is a substance that can donate H+ ions. The acidity of the substances is…

Q: Which of the following is the example(s) of acid-base reaction? H H `H H -Br II IV OH H-CI OH

A: Acid- The species which is able to donate H+ ion.   Base-  The special which is able to accept H+…

Q: What is the [OH'] and pOH of 0.10 M кОН solution with рH - 13.0 Рон - 1.0; [ОН-] - 0.10 М ОРОН -…

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Q: Calculate the pOH of an aqueous solution at 25°C that is (a) 0.011 M in HNO3 , (b) 3.5 × 10-3 M in…

A: pOH of solution can be can be calculated as, pH=-log[H+]pH+pOH=14pOH=14-pH

Q: What is the pH of 0.03 M acid solution? The K, of the acid is 5x10-3? А. 1.5 В. 1.9 С. 2.0 D. 2.3

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Q: Calculate the [OH] in 0.2110 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2…

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Q: What is the pH of a solution with H30+ =4.5 × 10^-5  M? 5.4 6.2 11.0 4.3

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Q: What is the pOH of 0.020M HNO3

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Q: Calculate [H3O+] and [OH−] for each of the following solutions at 25 ∘C given the pH. pH= 11.31

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Q: What is the ph of a solution with (H3O)= 6.4 x 10- 7th power

A: The concentration of hydronium ion is provided, i.e. [H3O+]=6.4 x 10-7 pH of the solution=?

Q: What is [OH ] in a 0.0058M HI solution?

A: The dissociation of HI takes place as,                                             HI (aq) ---->…

Q: Given Kb of OCl- is 3.5x10^-7 M. Calculate the pH of 0.1M NaOCl solution at 25°C.

A: Given, Kb of OCl- is 3.5x10^-7 M .  The pH of 0.1M NaOCl solution at 25°C is:

Q: Determine the [H*]. [OH ]. and pH of a solution with a pOH of 13.48 at 25 °C. [H*] = (OH] = %3D pH =

A: Hi, as you have posted 2 questions and have not mentioned which one you want us to solve, hence we…

Q: A particular base has Kb= 4.4*10^-4. What is the pH of 0.35M solution of this base ?

A: Since the Kb value is less so the dissociation of base is very less and it is assumed that the…

Q: What is the pOH of a 0.013 M Ca(OH)2 solution.  12.11 1.89 12.41 1.59

A: The concentration of the calcium hydroxide is = 0.013 M The pOH of the solution is =?

Q: Calculate the pOH of a solution that contains 7.8 x 10-6 M OH⁻ at 25°C.

A: pOH can be calculated using the given formula.

Q: What is the pOH for a solution that has 1.5 mol of HF dissolved in 2.0 L of water? Ka HF = 6.6 x…

A: Given  Ka HF = 6.6 x 10-4  and  1.5 mol of HF dissolved in 2.0 L of water.  pOH of the solution has…

Q: A solution formed by dissolving an antacid tablet has a pOHof 4.82. Calculate [H+].

A: Given that the pOH of solution is 4.82 .   pH can be calculated as follows:

Q: Calculate the pOH of a solution that results from mixing 41.4 mL of 0.11 M HBrO(aq) with 33.1 mL of…

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Q: A solution with a pOH of 11.70 has an [H3O+] of

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Q: a strong base Pe(OH)2 solution with (2.25x10^-4) M. Assume that the autoprotolysis of water does not…

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Q: The pOH of a solution is 9.05. What is the H* concentration in the solution?

A: [OH-] = 10-pOH  [H+].[OH-] = 10-14  [H+] = 10-14/ [OH-]

Q: Calculate the theoretical pH of the solution please 0.100 M aluminum nitrate Hydrated aluminum ion…

A: Al^3+ solution is slightly acidic in nature. This is because Al^3+ has very high ionic potential.…

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.