What is the pOH if a solution composed of 60mL of  0.0012M HCl and 200 mL of 0.0005M NaOH?

Q: What is the pHpH of an aqueous solution with [H3O+] =[H3O+] = 6×10−12 MM ? Express the pH…

A: The Formula to calculate pH is pH = - log [H3O+]

Q: What is the PH of a solution in which 15 mL of 0.01M NaOH has been to 25 mL of 0.01M benzoic acid…

A:

Q: 1. Which of the following changes with a change in molarity of a particular weak acid. I. pH of the…

A: Acid dissociation constant is a temperature dependent term.

Q: A 15.0 mL of 0.100 M HCl is mixed with 30.0 mL of 0.500 M NaOH. Which of the following is true?…

A:

Q: In a solution with OH- concentration of 3.0x10^-5 Match the following values that correspond to the…

A:

Q: Which one is correct? What is the [H3O+] in a solution with pH=8? 10+8 M 10-8 M 8.0 M 6x10-8 M…

A: Given, pH = 8 PH is defined as negative logarithm of concentration of [H+] ion.

Q: The Kw for water at 0 °C is 0.12 × 10-14 M². Calculate the pH of a neutral aqueous solution at 0 °C.…

A: In this question, we have to calculate the pH of a Neutral solution at 0°C when Kw for water at 0°C…

Q: Calculate the [OH-] of each aqueous solution with the following [H3O+], and then identify the…

A: pH : it can define have the negative logarithm of H+ ion or H3O+ concentration. When pH > 7…

Q: pH = –0.36  [H+] =  ____ M [OH - ]  = _____ M   b pH = 9.40  [H + ] =  _____ M  [OH - ] =…

A:

Q: HC4C3N2O3

A: Dear student I have given answer to your question in the image format.

Q: Which of the following statements is false regarding a solution of 1.0 M HNO3? [H+]=1.0M pH=0…

A: 1.0 M HNO3 HNO3 (aq)------> H+ (aq)+ NO3- (aq) pH = - log [H+] Here , [H+] = 1.0 M

Q: You are given 30 Calculate the values of both pH and pOH of the following solutions: pOH pH 0.020M…

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Q: pH and pOH

A: MMoles of NaOH = M × V     = 5.0×10-3 × 350  = 1.75 mmol After adding water, Concentration of  NaOH…

Q: 4. Calculate the value of [H3O'Jand [OH] in each solution: a. 0.0001 M NaOH b. 0.0001 M HCI

A:

Q: Which of these weak acid solutions has the greatest percent ionization? 0.500 M HF 2.50 M HF…

A: The reaction taking place will  be  HF ----> H+ + F-  Since the acid is weak so Ka will be very…

Q: What is the percent ionization of a 0.36M aqueous solution of formic acid, HCHO2 that is also 0.08 M…

A: 0.36 M aqueous solution of formic acid is present in 0.08 M HCl. The Ka of formic acid is 1.7 * 10-4…

Q: What is the pH of a 4.21 x 10-5M KOH solutio

A: pH helps in the measurement of acidity and basicity of a solution.

Q: 0.10M NaC2H3O2 solution ?

A: pH is the negative logarithm of hydronium ions. The acidic, basic and neural character of the…

Q: A 0.202 M solution of HX has a pH of 4.90 at 25°C. What is the value of Ka for HX? (the answer…

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Q: What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200M HCl solution?

A:

Q: A comic book villain is holding you at gun point and is making you drink a sample of acid. He gives…

A: Strong acid with pH = 5 pH = -log [H+] [H+] = 10-pH = 10-5 = 1x10-5 M [H+] =1x10-5 M Strong base…

Q: . pH = 7.40 (the normal pH of blood) pH = 15.3 pH = ‐ 1.0 pH = 3.20 pOH = 5.0 pOH = 9.6

A: 1. Given that the pH of solution is 7.40. If pH of the solution is greater than 7, then it is basic.…

Q: Ascorbic acid (Vitamin C, CHO) is a weak diprotic acid, with K = 6.8x10^-5 and K = 2.7x10^-12. What…

A: Let’s calculate the concentration of ascorbic acid Given amount = 13.6 mg Molar mass of ascorbic…

Q: How many mL of 0.2 M hydrochloric acid is required to neutralize 100 mL of 0.8 M KOH?

A: Given : Concentration of hydrochloric acid i.e HCl = 0.2 M Concentration of KOH = 0.8 M And volume…

Q: In a solution with OH- concentration of 3.0x10^-5 Match the following values that correspond to the…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: What mass of HNO3 is needed to make 315.0 mL of a solution with a pH of 2.27?

A: Consider the given information is as follows; Volume of the solution = 315.0 mL = 0.315 L…

Q: Calculate the pH at one-half the equivalence When 8.30 mL of 0.250M KOH is added to 35.0 mL of…

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Q: What is the percent ionization of a 0.68M aqueous solution of HF that is also 0.09 M HCl? The Ka of…

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Q: pH IV A solution has a [H+] = 1x 10-9. What can you conclude about this solution? Check all that…

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Q: A solution that is 0.10 M in NH3 and 0.10 M in NH4Cl. The Kb of ammonia is 1.8x10-5. What is the…

A: Given, 0.1 M NH3 and 0.1 M NH4Cl

Q: For a certain diprotic acid, the pH at one half the volume to the first equivalence point is 4.15…

A: The objective is to calculate the ka1 and ka2 to the following data. Given that For a diprotic acid…

Q: Calculate [H+] for each solution A.) pH=8.55 B.) pH = 1.22

A: pH = -log[H+] [H+] = 10-pH

Q: solution of 3.71×10-3 M potassium hydroxide? pOH =  B.) What concentration of sodium hydroxide is…

A: Potassium hydroxide(KOH) is strong base. And strong base dissociated completely [OH-] = 3.71 ×10-3 M…

Q: how would the pH of a 0.005M acetic acid compare to pH value 0.005 M HCl

A: Ch3COOH is a weak acid so it will not give More H+ .it will give H+ upto 5%. [H+]= √kaC Ka is…

Q: A solution is made from 0.45M NH3 and 0.44 M NH4CI. What is the pH if the Kh for NH3 is 1.8x107…

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Q: a) Calculate the degree of ionization of a 0.75 M HF (hydrofluoric acid) b)  the same solution that…

A: Ans a)

Q: of the elements indicated on the periodic table shown above, which forms the weakest binary acid, H…

A: A question based on periodic trends that is to be accomplished.

Q: A healthy individual has a blood with [H+] = 4.87× 10–8. Question: What is his/her blood pH?

A: The pH of a solution is a measure of the molar concentration of hydrogen ions in the solution and as…

Q: If det cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater…

A: The pH is the measure of the concentration of H+ ions in the solution. This measures the acidity of…

Q: Which pH has a [H+] twice as concentrated as that of a solution whose pH is 9.28? 4.64? 5.42 4.72…

A: Use below formula for this question: PH = -log[H+]   [H+]---> concentration(molL-1)

Q: Calculate the number of moles of KOH in 6.50 mL of a 0.430 M KOH solution. What is the pOH of the…

A: 6.50 mL of KOH solution has a concentration of 0.430 M. We have to calculate the number of moles…

Q: What is the PH of a solution in which 15 mL of 0.01M NaOH has been to 25 mL of 0.01M benzoic acid…

A: Consider the reaction of NaOH with benzoic acid to form sodium benzoate is as follows;…

Q: Ka for HCN is 6.2 x 10-10. The pH of an aqueous solution of 0.10M of NaCN is?

A:

Q: The pH of a 1 M hydrofluoric acid (HF) solution is about 3 and the pH of a 1 M hydrochloric acid…

A: Given, pH of 1M HF = 3. pH of 1M HCl = 1.

Q: The pOH of a solution made by combining 150.0 mL of 0.10 M KOH(aq) with 50.0 mL of 0.20 M HBr(aq) is…

A:

Q: What isthe pH of 20.0 mL of 0.100 M HAc into 100.0 mL 20.0 mL of 0.100 M NaOH?

A: Given data :  20 ml. of HAc  having molar concentration 0.100 M and  20 ml. of 0.100 M NaOH  mix…

Q: Calculate the pOH of a soda water solution with pH = 6.20. Express your answer to the nearest…

A: Given:  pH = 6.20 To find pOH

Q: A pH of -1.0 is an H+ concentration of 10M not possible an H+ concentration of 1M an H+…

A: Given: pH = -1.0.

Q: What is the pH of a solution in which 15 mL of 0.13 M NaOH is added to 25 mL of 0.13 м НCI? pH

A:

Q: What volume (in mL) of 11.7 M HCl would be required to make 500.0 mL of a solution with a pH of 3.20

A: [ H+ ] = [ HCl ]

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.