Calculate the molar concentration of the acid if 19.28 of nitric acid was required to neutralize 44mL of 0.267M aluminium hydroxide

Q: 100.0mL of a 0.050M HNO2 solution is titrated with a 0.10M NaOH solution. How many mL of NaOH would…

A: Let the volume of NaOH = V mL pH = 3.39 Molarity of HNO2 = 0.050M Molarity of NaOH = 0.10 M

Q: If the volume of blood in a normal adult is 5.0 L, what mass of HCl can be neutralized by the…

A:

Q: Calculate the pH of a solution made by mixing 100.0 mL of 0.110 M NaBrO with 75.0 mL of 0.140 M…

A: Given: Concentration of NaBrO = 0.110 M Concentration of HBrO = 0.140 M Volume of NaBrO = 100.0 mL…

Q: Calculate the pH of the resulting solution when 350.0 mL of .400 M HCl is mixed with 35.0 mL of…

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Q: A few mL of 0.800M HCl are added to 20mL of 0.800. NaC2H3O2. Will the initial pH of the 0.800M…

A: pH is used to determine the concentration of hydronium ion. pH for acid is less than 7. pH for base…

Q: Calculate the pH of a solution made by mixing 25.00ml. of 0.1056M HCI with 13.23ml of 0.1138M NAOH…

A: The acid solution is the solution in which loss of proton takes place and the pH of the solution is…

Q: How many milliliters of acetic acid with a concentration of 10M should be added to a liter of 0.09M…

A: Value of pH is used to calculate acidity or basicity of a solution. pH value of a solution at room…

Q: A student takes 93.3 ml of a 0.0363 molar KOH solution and dilutes it to a final volume of 6,143.2.…

A: Given, Initial volume of solution = 93.3mL = 0.0933L. Final volume of solution = 6,143.2mL =…

Q: Calculate the pH when (a) 24.9 mL and (b) 25.1 mL of 0.100 M HNO3 have been added to 25.0 mL of…

A: Part a: Number of moles of nitric acid = 0.0249 L × 0.1 M = 0.00249 mol Number of moles of KOH =…

Q: Calculate the pH when 19.15 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The neutralization reaction is given below.

Q: Calculate the pH of a mixture containing 0.266 mol HBz and 0.124 mol NaBz dissolved to 500.0 mL with…

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

Q: what is the pH of buffer solution containing 10.0g ammonium chloride to 250 mL of 1.0M ammonium…

A:

Q: Calculate the molar concentration (M) of NaOH if 25.00 mL of NaOH required 36.68 mL of a 0.9500M…

A: Hcl+NaOH---->NaCl+H2O Neutralization reaction  M1V1/n1=M2V2/n2

Q: Calculate the pH of a solution obtained by mixing 449 mL of0.17 M nitric acid with 405 mL of 3.6 x…

A: Since both the acid and base are strong in nature  Hence they will react until one of them gets…

Q: A 0.015 M solution of a weak acid, HA, is 17% dissociated. Calculate the Ka of the acid.

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Q: Calculate the concentration of phosphoric acid in a solution if 25.0 ml of that solution required…

A: The balanced equation can be shown below

Q: Determine the pH of the resulting solution when the following two solutions are mixed: 40.0 mL of…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Addition of 0.297 moles of nitric acid will: (Assume that the volume does not change upon the…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: 25.00ml of 0.5M hydrobromic acid solution is titrated with 0.455M potassium hydroxide solution. what…

A: A neutralization reaction can be described as a chemical reaction in which acid and base reacts…

Q: Calculate the pH when 148.5 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

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Q: Calculate the molar concentration of the acid if 27.20mL of nitric acid was required to neutralize…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: Calculate the pH at the stoichiometric point when 75 mL of 0.099M propionic acid is titrated with…

A: Moles of propionic acid = 0.075L*0.099 = 0.0074Mole (75mL= 0.075L) Mole acid (0.0074Mole) = moles of…

Q: Calculate the pH when 23.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: The volume of 0.150 M KOH is 23.0 mL. The volume of 0.300 M HBrO is 20.0 mL. The dissociation…

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH when 60.0 mL of 0.150 M HNO, is mixed with 40.0 mL of 0.250 M LIOH. 3.

A: HNO3 + LiOH  = H2O + LiNO3GIVENNumber of mmol HNO3 present initially=(60mL)×(0.150M) = 9mmolLiOH…

Q: Calculate the pH of solution prepared by dissolving 0.10 mol of NH.Cl and 0.40 mol of NH; in…

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Q: Calculate the pH when 25.36 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: Total volume of the solution (VT) after mixing the 25.36 mL of 0.100 M NaOH to 30.0 mL of 0.100 M…

Q: The equation Hln = H + In means? آختر احدى الدجابات A. The medium is acidic or basic B. Which form…

A: Hln   = H+  + ln- If acid is added then according to Le-Chatelier’s principle, the reaction will…

Q: Calculate the pH when 77.0 mL of 0.250 M HCI is mixed with 40.0 mL of 0.150 M Ca(OH):.

A:

Q: Calculate the pH when 29.91 mL of 0.2628 M carbonic acid is mixed with 10.1 mL of 0.1448 M NaOH.

A: For carbonic acid, 29.91 mL of 0.2628 M carbonic acid Ncarbonic acid  = n- factor × M…

Q: Calculate the expected pH based on how the solution was prepared, again allowing for any dilution…

A: pH of a buffer solution can be calculated by using Henderson Hasselbalch equation, according to…

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: Quinine (C20H24O2N2) is a water-soluble base that ionizes in two stages, with Kb1 5 3.31 × 10-6 and…

A:

Q: Calculate the pH of a solution obtained by mixing 438 mL of 0.14 M  nitric acid with 385 mL of…

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Q: Calculate the pH of a solution containing 200ml of 0.01M NaOH and 8ml of 0.25M of acetic acid.

A: Answer :-  The pH of a solution containing 200ml of 0.01M NaOH and 8ml of 0.25M of acetic acid =…

Q: Calculate the pH when 54.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Calculate mole of each substance then applied neutralissation reaction. limiting reagent is HBRO and…

Q: A1 liter solution is made by adding 0.5983 moles NaH2PO4 and 0.5456 moles NazHPO4. What will be the…

A:

Q: 10010 ml, 0.1M HcL is udded to 100 ml of asalFion Which IS 0.1 M both in HOAC and NAOAC. By how many…

A: The questions are based on the concept of PH calculations. we have to determine how much by pH…

Q: 0.272 g of a monoprotic acid (Mw = 189 g/mol) is dissolved in water to produce 25.0 mL of a solution…

A: Given, Mass of monoprotic acid (HA) = 0.272 g Molar mass of monoprotic acid = 189 g/mol Volume of…

Q: If you have 500 mL of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of…

A:

Q: Determine the pH of the solution obtained if 30 mL of 0.075 M ethylamine is titrated with 0.15 M HCI…

A: The balance equation is given below, Calculate the number of moles of ethylamine: 1 L = 0.001 mL…

Q: 18. Calculate the pH of a solution created by mixing 50.00 mL of 0.200 M HF with 25.00 mL of 0.250 M…

A: Given solution is acidic buffer  So use acidic buffer equation to get PH  PH= 3.49

Q: You have been observing an insect that defends itself from enemies by secreting a caustic liquid.…

A: The relation given by Henderson Hasselbalch for calculating the pH of the weak acid solution is…

Q: Calculate the pH of a solution formed by adding 8.00 grams of solid sodium azide, NaN₃, to 210.0 ml…

A: Molarity of Sodium Azide = 0.230 M Volume of Solution = 210.0 mL amount of sodium azide = 8 g Molar…

Q: calculate the pH of a solution prepared by mixing 456mL of 0.10M HCl with 285 mL of 0.15M NaOH.

A: The pH depends on -log of concentraion of H+ ion present in the solution.so first of all we have to…

Q: When 40.00 mL of a 0.1107 M of formic acid (HCOOH) is titrated with 18.22 mL of 0.1218 M NaOH,…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 39.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: The PH can be calculated as follows

Q: Calculate the pH when 25.0 mL of 0.150 M HNO3 is mixed with 40.0 mL of 0.250 M LIOH.

A:

Q: 35.75 mL of 0.500 mol/L KOH was needed to reach the endpoint in a titration of 25.00 mL HCl.…

A: It is an acid-base titration reaction of strong acid (HCl) with strong base (KOH)

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.