Answered: What volume of 0.05 M NAOH must be…

What volume of 0.05 M NAOH must be added to reach the final equivalence point in the titration of 30.0 mL of 0.1OM HCN? NaOH(aq) + HCN(aq) → H2O(1) + NaCN(aq)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 44QAP: A 50.0-mL sample of NaHSO3 is titrated with 22.94 mL of 0.238 M KOH. (a) Write a balanced net ionic...

See similar textbooks

Related questions

Q: If 20.0 g of NaOH is added to 0.750 L of 1.00 M Cd(NO:)2, how many grams of Cd(OH)2 will be formed…

A: Consider the given information is as follows; Mass of NaOH = 20.0 gVolume of CdNO32= 0.750…

Q: A 0.9600 M NaOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was…

A: (i) The initial concentration of NaOH = 0.960/4 = 0.2400 M. From the given table the volume of NaOH…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A: Answer In the titration reaction of oxalic acid and sodium…

Q: y titration, it is found that 34.9 mL34.9 mL of 0.103 M NaOH(aq)0.103 M NaOH(aq) is needed to…

Q: Acetic acid reacts with sodium hydroxide in the following fashion. HC2H3O2(aq) + NaOH(aq) →…

Q: Potassium sorbate,KC H,O, (molar mass 150. g/mol) is commonly added to diet soft drinks as a…

A: Solution: Dissociation expression is a dissociation constant ( equilibrium constant). For acid…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A: A numerical problem based on quantitative analysis, which is to be accomplished.

Q: 1) Potassium permanganate solutions used in oxidation-reduction titrations are often standardized…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: A 10.0 sample of vinegar (acetic acid) is titrated with a 0.495 M NaOH solution. End point is…

Q: A 31.00 mL sample of an unknown H3PO4 solution is titrated with a 0.120 M NaOH solution. The…

A: Given, Volume of H3PO4 = 31.00 mL = 0.031 L (1 mL =0.001 L) Volume of NaOH = 26.43 mL = 0.02643 L…

Q: In one experiment, a 34.9 ml sample of 0.188 M phosphoric acid was titrated with a 0.22 M solution…

Q: A 5.00 mL sample of 0.25 M HBr solution is titrated with 0.35 M NaOH. What volume of NaOH is…

A: We should equal equivalent of both acid and NaOH ion to volume of NaOH Equivalent =…

Q: An unknown volume of 0.518 M HNO3 (aq) was titrated with 0.882 M NAOH (aq). It took 24.2 mL of the…

A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: The endpoint in a titration was reached when 23.5 mL of a 0.0100 M solution of NaOH was added to…

A: The given neutralization reaction is as follows: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) The molarity…

Q: A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated…

A: A saturated solution of solid calcium hydroxide, Ca(OH)2, is made by dissolving in enough water. Now…

Q: Assume you titrated to the endpoint 0.10 moles of HA (weak, monoprotic acid) with a solution of…

Q: A 0.9600 M NaOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was…

A: As you have posted multiple questions in a single request, we will solve the first question for you.…

Q: A mixture containing 0.10 M KBr(aq) and 0.22 M NaF(aq) is electrolyzed. What is formed and why?

A: During electrolysis, oxidation takes place at anode and reduction takes place at cathode. Hence all…

Q: A 112 mL sample of an unknown concentration of the base barium hydroxide requires 177 mL of 2.44 M…

A: According to the balanced equation given above, 2 moles of HCl require 1 mole of Ba(OH)2. So, the…

Q: You perform the following titration. The concentrations and amounts of your reactants are listed…

A: Intrdouction : We have to calculate the pH of solution .

Q: The titration of 25.00 mL of an unknown concentration of H2SO4 solution requires 44.58 mL of 0.42 M…

Q: For a tablet containing 1000 mg of vitamin C, calculate the minimum concentration of the NaOH…

A: Given that : Mass of vitamin C = 1000mg = 1000mg×1g/1000mg = 1.00g Volume of NaOH used to…

Q: In a titration, it is found that 50 mL of 0.30M KOH will just neutralize 15 mL of an HCl solution.…

A: Given data, Volume of KOH = 50 mL Concentration of KOH = 0.30 M Volume of HCl = 15 mL

Q: The titration of 36.7 mL of sulfuric acid solution requires 43.2 mL of standard 0.236 M sodium…

Q: An acid-base titration is used to standardize a solution of NaOH. A student adds 25.00 mL of a…

A: KHP + NaOH→NaKP + H2O At equivalence point No. of moles of KHP=No. of moles of NaOH

Q: In a different titration experiment, it took 27.2 mL of a 0.102 M solution of NaOH to titrate 20.00…

A: Answer = 0.139 M

Q: A solution of tartaric acid (H2C,H,O6) with a known concentration of 0.155 M H2C,H,O6 is titrated…

A: Given, H2C4H6O6+2NaOH→Na2C4H4O6+2H2OK. Concentration of tartaric acid = 0.155M Concentration of…

Q: Calculate the molar concentration of H3O+ ions and the pH of the following solutions: (a) 25.0 cm3…

A: Given, (a). 25.0 cm3 of 0.144 M HCI(aq) was added to 25.0 cm3 of 0.125 M NaOH (aq) (b). 25.0 cm3 of…

Q: A 0.9600 M NaOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was…

Q: A titration of 38.0 mL of a sulfuric acid (H₂SO₄) solution of unknown concentration with a…

A: Given: Volume of H2SO4 (V1) = 38.0 mL Concentration of Ba(OH)2 (M2) = 1.55 M Volume of Ba(OH)2 (V2)…

Q: A permanganate solution is standardized by titrating it with a 0.1712 M SO,2- solution. The balanced…

Q: The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of…

A: Acid-base titration: Titration is a method to determine the concentration of unknown acid by using…

Q: A 25.00 mL sample of acetic acid (CH3COOH) is titrated to the equivalence using 31.08 mL of 0.1978 M…

Q: In a different titration experiment, it took 26.48 mL of a 0.155 M solution of NaOH to titrate 20.00…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A: The reaction of oxalic acid and NaOH – H2C2O4 +2NaOH →Na2C2O4 + 2H2O

Q: If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being…

A: For NaOH, Molarity, M1 = 1.0 M = 1 mol L-1 Volume used, V1 = 29 mL = 29 x 10-3 L…

Q: titration, if 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point.…

A: The solution is as follows:

Q: Acid-base titrations are an important method of chemical analysis. If you use 32.45 mL of HCl to…

A: From the balanced equation: Number of moles of Na2CO3 = 2 × Number of moles of HCl Number of moles…

Q: A 25.0 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.105 M NaOH (aq). It took…

Q: A solution of citric acid (F3C6H507) with a known concentration of 0.200 M H3C6H507 is titrated with…

Q: The endpoint of a titration is reached when 25.6 mL of a 0.100 M solution of Ca(OH)₂ is added to…

Q: KHP (potassium hydrogen phthalate, KHC8H4O4

A: Molarity = Moles of solute/ volume of solution (in L) Moles = Mass in gm/molar mass

Q: A buffer was prepared by mixing 147.78 g (CH3)3N and 272.37 g (CH3)3NHCI in a solution with a total…

Q: In a titration of KOH, 0.0725 g of KHP is weighed into a flask and dissolved in deionized water. The…

A: Molar mass of KHP is 204.22 g/mol. Calculation of no. of mol of KHP: Since KHP is a monoprotic…

Q: Question attached

A: To calculate the grams of Ni(OH)2 produced in the below reaction 2NaOHaq+NiNO32aq→NiOH2s+2NaNO3aq…

Q: A solution of Ba(OH)2 is titrated into a solution of HOI. Calculate the volume of 0.140 M Ba(OH)2…

A: Interpretation - To determine the volume 0.140 M Ba(OH)2 (aq) needed to reach the equivalence point…

Q: A volume of 15.00 mL of NaOH was titrated with 11.34 mL of 0.1311 M HCl. Calculate the molarity of…

Q: A 20.00-mL sample of aqueous oxalic acid, H2C2O4, was titrated with a 0.09113-M solution of…

A: Given: Volume of Oxalic acid: 20.00 mL The concentration of Potassium permanganate: 0.09113 M The…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A: Molarity of a solution =Number of moles of soluteVolume of solution in LNaOH + H2C2O4 →Na2C2O4 + 2…

Q: A. What is the pH of an aqueous solution with a hydrogen ion concentration of…

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

Concept explainers

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.

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A solution of HClO4 was standardized by dissolving 0.4008 g of primary-standard-grade HgO in a solution of KBr: HgO(s) + 4Br- + H2O à HgBr42- + 2OH- The liberated OH- consumed 43.75 mL of the acid. Calculate the molar concentration of the HClO4.
This is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid? The reaction is: H3PO4 (aq) + 3 NaOH (aq) → Na3PO4 (aq) + 3 H2O (l)
A 11.50 mL sample of HBr is titrated with 23.50 mL of a 0.80 M solution of NaOH to endpoint. What is the molarity of the HBr solution? Given: HBr (aq) + NaOH (aq) ---> H2O (l) + NaBr (aq) Express molarity as M
During the titration of 50.0mL of 0.1098M HCl using a standardized 0.0750M NaOH solution, what would be the pH of the solution (round off to 2 decimal points) after the addition of: a.) 0.00mL NaOH total volume? b.) 50.0mL NaOH total volume? c.) 75.0mL NaOH total volume? d.) 100.mL NaOH total volume?
. A 0.125 g sample of a monoprotic acid (HX, one proton/H+) of an unknown molecular weight is dissolved in water and titrated with 0.1003 M KOH. The endpoint is reached after adding 20.77 mL of base. What is the molecular weight of the unknown acid? HX (aq) + KOH (aq) → H2O (l) + KX(aq)
A solution of HCl with a volume of 25.00 mL is titrated to the endpoint, with 0.250 M NaOH. If it takes 34.56 mL of NaOH, what is the originial concentration of HCl in the solution?: HCl (aq) + NaOH (aq) ---> H2O (l) + NaCl (aq)
Consider the 25.0 mL portion of pH=4.45 buffer solution prepared as described in question 4. Calculate the buffering capacity of it for the hydrochloric acid of known concentration (M = 0.123 mol/L). Hint: you are calculating how much of the strong acid (HCl in this case) you can add to the buffer portion before you see a significant pH change, so start with deciding which component of the buffer will be the buffering species against the strong acid. Then calculate how much of that species is present in the 25.0 mL portion of this buffer. For the sake of these calculations, consider the buffering capacity to be the maximum volume of the strong acid that can be added to the portion of your buffer before the buffering species in it is completely used up, and the buffer is ‘overwhelmed’. Provide the answer in millilitres, mL. Don't include units.
Maleic acid (H2C4H2O4, represented by H2M) is the precursor of malic acid widely used in industry. food as an acidulant and in the pharmaceutical industry it is used in the treatment of wounds. This acid can be determined by neutralization titration. Answer the items below about this determination. a) Considering a 15.0 mL sample of maleic acid-based product used in industry, determine the maleic acid concentration, in mol/L, in the sample knowing that 21.7 mL of a solution of 0.1120 mol/L NaOH for complete neutralization of this acid. How many grams of maleic acid were in the sample analyzed and what is its percentage (%, m/v) in the sample? [Answer; m=0.1405 mol/L; percentage = 0.9365%] NaOH(aq) + H2M(aq) ----> Na2M (aq) + H2O(l) b) And Suggest an appropriate indicator for the titration of this acid by looking at the titration curve profile below (image)
From the titrations below, calculate the molarity of the NaOH solution in each of the f ollowing? Make sure you balance the equations. a) NaOH + HCl → NaCl + H2O 32.00 ml of NaOH is required to completely react with 25.00 ml of 0.150 M HCl. ___________ b) NaOH + H2SO4 → Na2SO4 + H2O 42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H 2SO4 . __________
QUESTION 6 The following equation describes the titration of KHP with NaOH: HKC8H4O4 (aq) + NaOH (aq) → NaKC8H4O4 (aq) + H2O (ℓ) "KHP" If 0.568 g of KHP is used, how many moles of KHP are present? Report your answer to 3 significant figures.
1 points QUESTION 9 Calculate the pH during the titration of 20.00 mL of 0.1000 M C6H5COOH(aq) with 0.2000 M NaOH(aq) after 4.77 mL of the base have been added. Ka of benzoic acid = 6.5 x 10-5.
What is the molar mass of an unknown triprotic acid if 0.0913 g of the acid is titrated, and the first equivalence volume is reached after having delivered 19.32 mL of a 0.1000 M KOH solution? Group of answer choices 94.5 g/mol 47.3 g/mol 142 g/mol 21.2 g/mol 15.8 g/mol