What is the pH of a solution that is 1.67x10-5M H+?a. 4.8b. 5.2c. 0.22d. 10.2

Q: A concentrated HCl solution contains 36.0% HCl (density of 1.18 g/mL). How many liters are required…

A: pH: The acidity of the solution is given in the term of pH, it is given by negative logarithm of…

Q: 9. If 50 mL of 0.1 M NAOH was added to each beaker, which resulting solution would have the lowest…

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Q: Order the following solutions from lowest pH to highest pH. i. O.10M NacIO ii. 0.10M KBr iii. 0.10M…

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Q: A certain weak base has a ?b of .8.40×10−7. What concentration of this base will produce a pH of…

A: Assuming the weak base is monoprotic which can be written as BOH. Hence the dissociation reaction of…

Q: Calculate the pH of each of the following strong acid solutions:(a) 8.5 x 10-3M HBr, (b) 1.52 g of…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: Consider a HCl solution that has a pH of 4.70. a) Calculate the concentration of HCl.  b) Identify…

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Q: Q3// Grams of Sodium Formate required to add to 400ml of o.1M Formic acid to make the pH of solution…

A: The given solution is a buffer of Formic acid and Sodium formate. The pH of a buffer solution is…

Q: Calculate the pH of a formic acid solution that contains 1.35% formic acid by mass. (Assume a…

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Q: which assumption can't be applied in the calculation of the pH of this solution? (a) that the…

A: pH is the measure of the concentration of the H+ ions in the solution. It can be acidic, basic, and…

Q: I'm not sure how to do this question

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Q: 6) a solution Boric Acid : %3D Calculate PH(? >eguilibri ?) um constant

A: H3BO3  + H2O  → H3O+  +  H2BO3- Given that,[H3BO3] = 0.200 M [H2BO3-] = [H3O+] = 1x10-5 M Calculate…

Q: 6. Which solution has the highest pH? A. 0.10 M HCIO4 (aq) B. 0.10 M HBrO4 (aq) C. 0.10 MHCI0(aq) D.…

A: pH is defined as negative logarithm of hydrogen ions

Q: 13.6 mL of an HCl(aq) solution with a pH of 2.65 are mixed with 14.2 mL of another HCI(aq) solution…

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Q: Grams of Sodium Formate required to add to 400ml of 0.1M Formic acid to make the pH of solution by…

A: The reaction can be given as follows: HCOOH(aq)+NaOH(aq)→HCOO-Na+(aq)+H2O(l) Molarity of formic acid…

Q: Part A If 15.0 mL of glacial acetic acid (pure HC2H3O2; K₂ = 1.8 × 10−5) is diluted to 1.70 L with…

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Q: Order the following solutions from lowest to highest pH: (i) 0.10 M NaClO, (ii) 0.10 M KBr, (iii)…

A: pH is used to determine the concentration of hydronium ion. The formula is represented as follows:…

Q: What quantity of moles of glucose (C₆H₁₂O₆) in 0.500 L of a 0.400 M solutions?     The pH of a basic…

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Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

A: Henderson-Hasselbalch equation The equation that is used to find the pH of a buffer solution is…

Q: For each strong acid solution, determine [H3O+], [OH-], and pH.a. 0.25 M HClb. 0.015 M HNO3c. a…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall only…

Q: Diluted sulfuric acid has a density of 1.3 g / ml and contains 39% by mass of H2SO4. a) What is the…

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Q: (References) A typical vitamin C tablet (containing pure ascorbic acid, H2C6H606) weighs 500 mg. One…

A: The question is based on the concept of equilibrium. we have been given a weak acid ascorbic acid.…

Q: 3 60.0 ml of NaOH, the pH of the resulting solution is greater than 7. g 20.0 mL of NaOH, the pH of…

A: Mmol of formic acid = M × V     = 0.60 × 40 = 24 mmol After adding 60 mL of NaOH,  Mmol of NaOH =…

Q: A chemist dissolves 890. mg of pure barium hydroxide in enough water to make up 110. mL of solution.…

A: Mass of barium hydroxide = 890 mg  Volume of solution = 110 ml Temperature = 25 °C  pH of the…

Q: If a acidic solution with a pH of 4 is completely neutralized, by how much will the hydronium ion…

A: We have to check whether the concentration will increase or decrease if pH goes from 4 to 7 .

Q: A solution containing 2.60 x 103 moles of HCl and 3.32 x 10~³ moles of NaOH into a container and…

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Q: 1-L unbuffered solution needs the pH adjusted from 12.5 to 3.6. How many mL of 4 holar HCl solution…

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Q: in a solution are 0.01 moles of NH4OH and 0.1 moles of NH4Cl.pH of this solution is: a) 7 b) 8 c) 9…

A: Henderson-Hasselbalch equation The equation that is used to find the pH of a buffer solution is…

Q: A chemist dissolves 846. mg of pure hydrobromic acid in enough water to make up 210. mL of solution.…

A: Given: Mass of HBr  = 846.0 mg = 0.846 g Volume of HBr solution = 210.0 mL = 0.210 L Molar mass of…

Q: 7.30×10−7. What concentration of this base will produce a pH of 10.14?

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Q: A substance ‘X’ used in the kitchen for making tasty crispy pakoras and is also an Ingredient of…

A: The antacid active ingredient is sodium-bicarbonate which makes pakoras tasty and crispy. When…

Q: How many mL of a 0.092 M NAOH solution would be required to neutralize (bring it to pH 7.0) a 50 mL…

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Q: pH

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Q: A certain weak base has a ?b of 8.40×10−7. What concentration of this base will produce a pH of…

A: Weak base dissociated less in solution

Q: For each strong acid solution, determine (H;O'], [OH¯], and pH. a. 0.25 M HCI b. 0.015 M HNO, c. a…

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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: For a 0.40 M solution of HCIO4, calculate: [H+], pH, pOH, and [OH"] Determine all pH and pOH values…

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Q: Q3// Grams of Sodium Formate required to add to 40oml of o.1M Formic acid to make the pH of solution…

A: Given that: molarity of formic acid = 0.1 M Volume of solution = 400 mL Ka = 1.74×10-4 M.wt of…

Q: A certain weak base has a ?b of 7.90×10−7. What concentration of this base will produce a pH of…

A: As per the given information  certain weak base has a kb is 7.90×10-7. pH=10.03 The chemical…

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH?…

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Q: Calculate the pH of each of the following strong acid solutions:(a) 0.0167 M HNO3, (b) 0.225 g of…

A: To calculate pH of each of strong acid solutions: (a). 0.0167 M HNO3

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Q: A chemist dissolves 461. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

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Q: The PH of a solution of HCL in water is found to be 2.50.what volume of water would you add to 1.00L…

A: The given value of pH = 2.50 is present in 1 L of water . As we know as the pH value increases the…

Q: ou are given the following ; KBr, NH3, NaOCl, NH4Cl they are all 1 M aqueous solutions some other…

A: The given four compounds are KBr, NH3, NaOCl, NH4Cl. The concentration of each compound in the…

Q: A certain weak base has a K, of 7.20 × 10-7. What concentration of this base will produce a pH of…

A: Given  Kb = 7.20 x 10-7 pH = 10.14  we know  pH + pOH = 14  pOH = 14 - 10.14 = 3.86 and   [OH-] =…

Q: A certain weak base has a K, of 8.80 x 10-7M. What concentration of this base will produce a pH of…

A: Given data: The Kb value of weak base = 8.80×10-7. The pH of the weak base = 10.28. To calculate:…

Q: op your selection from the following list to complete the answer: NaF HI HF HCI, KCI, H,NNH3…

A: Acidic solution has pH less than 7 Basic solution has pH greater than 7 and  neutral solution has pH…

Q: certain weak base has a  ?b  of  7.80×10−7.  What concentration of this base will produce a pH of…

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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.