A 38.05 mL aliquot of weak base that has a concentration of 0.577 M will be titrated with 0.39 M HCl. Calculate the pH of of the solution upon the addition of 14.02 mL of HCl. The Kb of the base is 2.2×10-6.

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and potassium…

A:

Q: Suppose a buffer solution contains Z moles of NaOH and 0.025 moles of its salt. The pH of the…

A: Given: Moles of salt = 0.025 mol pH of solution = 9.034 Kb  = 1.8 × 10-5

Q: Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer…

A: pH is used to determine the concentration of hydronium ion.

Q: The pH at the equivalence point where 50.00mL of 1.060M HIO is titrated with 0.300M NaOH solution is…

A: The concentration of hydroxide ion after mixing of HIO and NaOH is calculated as,

Q: What is not correct in computing for the buffer capacity, if an additional acid is added a. The…

A: Buffer capacity is the amount of acid or base that it can effectively neutralize.

Q: A 2.14-g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution…

A: Sodium Hypoiodite is NaIO. It is a base and therefore, we will symbolize it by 'B' as per the…

Q: When a 15.0 mL sample of a 0.315 M aqueous hypochlorous acid solution is titrated with a 0.481 M…

A: In this question, we want to determine the pH of the Solution after mixing of HClO with Ba(OH)2 You…

Q: An aqueous solution contains 0.461 M ammonla. Calculate the pH of the solution after the addition of…

A: The concentration of ammonia = 0.461 M = 0.461 mol/L (M = mol/L) The number of moles of hydrobromic…

Q: A 36.0 ml. sample of a 0.446 M aqueous hypochlorous acid solution is titrated with a 0.205 M aqueous…

A:

Q: A solution is prepared by adding 31.56 grams of NaCN and 22.30 grams HCN to 600.0mL of water. i.…

A: First Calculate mole of each NaCN and HCN by dividing Molar mass to mass. Use Acidic buffer equation…

Q: In another experiment, the student titrated of with 50.0 mL of 0.1M HC2H3O2 with 0.1M NaOH.…

A: We have given that  Titration of CH3COOH Vs  NaOH  Molarity of CH3COOH = M1 = 0.1M Volume of CH3COOH…

Q: In titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: We have to calculate the pH of solution.

Q: A solution of oxalic acid is used to titrate 17.11 mL of a 0.5003 molar: sodium hydroxide. If the…

A:

Q: Which of the following statement is incorrect regarding buffer solutions: O a Maximum buffer…

A: The solution is given below -

Q: In titrating 40.0 mL of 0.10M of HCI solution with 0.15 M of KOH solution, what would be the pH of…

A: Given that ,  HCl (acid) KOH (base) Molarity(Ma) = 0.10 M Molarity (Mb) = 0.15 M Volume (Va)…

Q: A 30.0 mL sample of 0.200 M HNO, solution is titrated with 15.0 mL of a 0.300 M LIOH solution.…

A:

Q: A solution that contains an equal number of moles of _____ will be a buffer solution.  a. HF and…

A: Buffer Solution is a water solvent based solution which consists of a mixture containing a weak acid…

Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: [References] Use the References to access important values if needed for this question. A buffer…

A:

Q: How many grams of solid ammonium chloride should be added to 0.500 Lof a 0.239 M ammonia solution to…

A: The given information is: Volume of the solution = 0.5 L Concentration of the solution = 0.239 M pH…

Q: The pH of a solution that contains 1.2M acetic acid and 0.920M sodium acetate is?

A: pH of weak acid = 4.63.

Q: A 50.000 mL aliquot of weak base that has a concentration of 0.285 M will be titrated with 0.684 M…

A: Given that,  Volume of 0.285 M weak base = 50.0 mL = 0.05 L Moles of weak base given = 0.285 M×0.05…

Q: The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with…

A:

Q: A 100.0 mL of 0.1 M HCI solution is mixed with a 50.0 mL of 0.1 M of KOH solution. The resultant…

A:

Q: . (a) Which is the stronger base—the basic form of the indicator cresol red or         the basic…

A: Indicators are substances whose solutions change color due to changes in pH. They are usually weak…

Q: Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to…

A:

Q: A solution is made by mixing 50.0 mL of a stock solution of 2.0 M K2HPO4 and 25.0 mL of a stock…

A: Buffer solutions: are defined as the aqueous solution which contains the mixture of the weak acid…

Q: Which of the following statement is incorrect regarding buffer solutions: O Buffer solutions are…

A: Buffer solution is the solution which resist the change in pH when small amount of acid or base is…

Q: Calculate the ph of at second equivalence point when 0.10M trisodium arsenate is titrated with 0.20…

A: trisodium arsenate, Na3AsO4(aq) is a deprotonated form of H3AsO4(aq), which is a tribasic acid. The…

Q: A solution containing 15.0mL of 4.00MHNO3 is diluted to a volume of 1.00L. What is the pH of the…

A: The given volume and molarity of HNO3 are 15.00 mL and 4.00 M. The given volume of diluted solution…

Q: The pOH of an acidic buffer is 9.725. What is the Ka of the acid if the ratio of [ionized] to…

A: pOH = 9.725  Ratio  = 1380

Q: Which of the following statement is incorrect regarding buffer solutions: OBuffer solutions are…

A: Buffer solution : It is a solution formed by weak acid and it's conjugate base pr vice-versa and…

Q: If a buffer solution is 0.280 M in a weak acid (?a=1.6×10−5) and 0.510 M in its conjugate base, what…

A:

Q: .623 g of NaC2H3O2 are placed in a solution of 0.105 M HC2H3O2 to make 1.00 L of solution. What is…

A: pH is negative logarithm of Hydrogen ion concentration

Q: Explain how the pH of a mixture of aqueous ammonium chloride and aqueous ammonium remains constant…

A: The solution that can resist the addition of the strong acid or strong base is termed as the buffer…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.11 M solution. The pH of the…

A: The concentration H3O+ of weak acid [H3O+] = Ka*C  where Ka is the dissociation constant, C is the…

Q: A 1.36 L buffer solution consists of 0.341 M propanoic acid and 0.120 M sodium propanoate. Calculate…

A: Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…

A:

Q: What is buffer solution?give the application of buffer with proper example?

A: A solution is made up of two components - solute and solvent. A solution can be heterogeneous and…

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: In a solution, when the concentrations of a weak acid and its conjugate base are equal, A. the…

A: pH of buffer solution of weak acid and salt of weak acid that is its conjugate base is given below.…

Q: A 20.0-mL sample of 0.200 M HBr solution is titrated with0.200 M NaOH solution. Calculate the pH of…

A: HBr  + NaOH  ------->  NaBr   + H2O millimoles of HBr = M x V = 0.2 x 20 = 4 mmol millimoles of…

Q: what is the pH?

A: Given :-  Concentration of weak acid = 0.250 M  Concentration of conjugate base = 0.450M  Ka = 5.9 ×…

Q: If 50mL of 0.10M NaOH is added to 50mL of 0.10M monoprotic weak acid, the resulting pH of the…

A: This can be calculated using Henderson -Hasselbalch equation

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.21 M solution. The pH of the…

A:

Q: 100 mL of 0.10 M HC1 is titrated with a solution of 0.10 M NAOH. After 20 mL of the NAOH solution,…

A: When acid and base react together and form salt and water this reaction is called a neutralization…

Q: Addition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition…

A: a) Given: Addition of phenolphthalein: No color change  Addition of bromthymol blue: Yellow color…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.07 M solution. The pH of the…

A:

Q: Calculate the PH of a buffer solution prepare with 0.14 M ammonia and 0.12 M ammonium chloride.…

A:

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0536 M HNO, to…

A: a.) When 0.00 mL HNO3 is added , there is only aziridine ( weak base ) in the solution so we would…

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.