20 g a sample of Ba(OH)2 is dissolved in 10 mL of 0.5 N HCL solution: The excess of HCL was titrated with 0.2 N NaOH. The volume of NaOH used was 20 cc. Calculate the percentage of Ba(OH)2 in the sample.

20 g a sample of Ba(OH)2 is dissolved in 10 mL of 0.5 N HCL solution: The excess of HCL was titrated with 0.2 N NaOH. The volume of NaOH used was 20 cc. Calculate the percentage of Ba(OH)2 in the sample.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.98E

See similar textbooks

Related questions

Q: A 15.0 mL solution of Sr(OH)2 is neutralized with 42.7 mL of 0.350 M HCI. What is the concentration…

A: The reaction involved is Sr (OH)2 + 2 HCl → SrCl2 + 2 H2O

Q: A student weigh out 2.795 g of potassium hydrogen phthalate (molar mass is 204.22 g/mol) to do a…

A: Given :- Mass of potassium hydrogen phthalate = 2.795 g Molar mass of potassium hydrogen phthalate…

Q: A 25.0 mL solution of HBr is neutralized with 14.2 mL of 0.105 M Sr(OH)₂. What is the concentration…

Q: By titration, it is found that 24.7 mL of 0.184 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: The reaction of HCl with NaOH is a neutralization reaction that forms NaCl and water as the…

Q: What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by…

A: Given,Final volume = 500.0 mlConcentration of HCl = 11.6 M

Q: Imagine your instructor gave you a solution of carbonic acid (H2CO3) and asked you to determine the…

A: The number of the moles of solute to the volume of solution in liters is known as molarity.

Q: A 25.0 mL solution of HNO₃ is neutralized with 20.4 mL of 0.250 M Ba(OH)₂. What is the concentration…

A: Given : volume of HNO3 = 25.0 mL Volume of Ba(OH)2 = 20.4 mL…

Q: Is BaF2 soluble in water, and if so, what ion is produced

Q: A 25.0 mL solution of HBr is neutralized with 16.5 mL of 0.105 M Sr(OH)₂. What is the concentration…

Q: By titration, it is found that 73.9 mL of 0.190 M NAOH(aq) is needed to neutralize 25.0 mL of…

A: Given :- concentration of NaOH = 0.190 M Volume of NaOH solution = 73.9 mL…

Q: A 25.0 mL solution of HBr is neutralized with 20.5 mL of 0.105 M Sr(OH)₂. What is the concentration…

A: Given: Volume of HBr solution = 25.0 mLVolume of Sr(OH)2 = 20.5 mLMolarity of Sr(OH)2 = 0.105 M

Q: A 1.146 g sample of weak acid is dissolved in 164.2 mL of water and titrated with 0.248 M NaOH to…

A: Given, mass of weak acid = 1.146 g Volume of weak acid = 164.2 mL Concentration of NaOH = 0.248 M…

Q: A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained…

A: Given, Volume of calcium hydroxide = 87.5mL Molarity of HBr = 0.0892 M Volume of HBr = 68.7 mL

Q: A 25.0 mL solution of HNO₃ is neutralized with 45.6 mL of 0.250 M Ba(OH)₂. What is the concentration…

Q: By titration, it is found that 24.5 mL of 0.173 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: The question is based on the concept of titration. We have to calculate concentration of…

Q: A 25.0 mL solution of HBr is neutralized with 14.5 mL of 0.105 M Sr(OH)₂. What is the concentration…

Q: By titration, it is found that 63.7 mL of 0.184 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Given, 63.7 mL of 0.184 M NaOH 25.0 mL of HCl

Q: If 26.92 mL of a solution of Ba(OH)2 requires 16.36 mL of a 1.247 M solution of HNO3 for complete…

A: Dilution is the method of reducing the concentration of the solvent in the solution by adding more…

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

A: The molar mass of KHP is 204.22 g/mol. The number of moles of KHP can be calculated by dividing the…

Q: 4) In a titration experiment, a 12.5 ml sample of 0.0175M Ba(OH)2 just neutralized 14.5 ml of HNO3…

A: We know M1=? V1=14.5ml M2= 0.0175M V2=12.5ml…

Q: The OH concentration in a 7.5 x 103 M Ca(OH)2 solution is x 10 12 M 1.30 x 10°M 7.5O х107м 100 x 102…

A: Given data, Concentration of Ca(OH)2 = 7.5 × 10-3 M

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: Calculate the molar concentration for H2 SO4 when 41 mL of it was completely titrated by 10.9 mL of…

Q: 1.46 g Potassium hydrogen phthalate requires 34.3 mL of 0.145M NaOH for neutralization, what…

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

Q: 2. Determine the volume of 0.250 M of NaOH required to neutralize 0.125 grams of dried KHP.

A: The reaction taking place between KHP (KHC8H4O4) and NaOH is- KHC8H4O4 (aq)+ NaOH (aq)→KNaC8H4O4…

Q: solution

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

Q: A 25.0 mL solution of HBr is neutralized with 10.7 mL of 0.230 M Ba(OH)2. What is the concentration…

A: Acid reacts with base to form salt and water. The given acid is HBr and base is BaOH2.

Q: 50.00 mL of a sulfuric acid solution, whose concentration is unknown, is titrated with 12.54 mL of…

A: Given: The Volume of sulfuric acid=50.00 mL=0.050 L Molarity of sulfuric acid=M mol/L The Volume of…

Q: A 25.0 mL solution of HNO₃ is neutralized with 24.1 mL of 0.125 M Sr(OH)₂. What is the concentration…

Q: The OH concentration in a 7.5 x 103 M Ca(OH)2 solution is 1.5x 102 M. 1.3x 10 12 M. 1.0x 107 M. 7.5x…

A: Given information, Concentration of Ca(OH)2 = 7.5*10-3 M Calculate : Concentration of OH- = ?

Q: What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by…

A: Given, 20.0 mL of concentrated (11.6 M ) HCl

Q: A 25.0 mL solution of HNO3 is neutralized with 19.7 mL of 0.125 M Sr(OH)2. What is the concentration…

A: Given : Volume of HNO3 solution = 25.0 mL Volume of Sr(OH)2 required = 19.7 mL Concentration of…

Q: A student performs a titration by filling the titrator with 0.75 M NaOH, and filling a beaker with…

A: Given data: Concentration of NaOH solution: 0.75 M, Volume of NaOH solution: 4.5 mL = 0.0045 L,…

Q: For the determination of acetic acid in vinegar, 1 mL of sample is taken, diluted to 100 mL and…

A: Acetic Acid is CH3COOH. Its molecular weight is:- 60.052 g/mol

Q: The following solutions are needed to be prepared for the titration procedure: 1. 20 mL of 2 M HCl…

A: The titration process wherein 1.0867 grams of Fe(OH)n was mixed with the 20 mL of 2 M HCl that you…

Q: By titration, it is found that 51.5 mL51.5 mL of 0.143 M NaOH(aq)0.143 M NaOH(aq) is needed to…

A: HCl and NaOH always react in equal equivalents or they react in equal moles.

Q: If 0.235 g of KHP (potassium hydrogen phthalate) require 15.51 mL of NaOH solution to neutralize it,…

A: For the neutralization number of mmols of NaOH = number of mmols of KHP Number of mols = Molarity x…

Q: By titration, it is found that 96.5 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of…

A: Given information:Volume of NaOH (V1)= 96.5 mLVolume of HCl (V2)= 25.0 mLMolarity of NaOH (M1)=…

Q: PART I Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by…

A: Number of moles of hydrochloric acid = concentration X volumeNumber of moles of hydrochloric acid =…

Q: A sample of KHP. KHCaH.Os, weighing 2.035 g is titrated with NaOH and backtitrated with HCI. NaOH…

A: Given: Mass of sample of KHP =2.035 g Volume of NaOH required =23.20 mL Volume of HCl required…

Q: A 25.0 mL solution of HCl is neutralized with 12.7 mL of 0.240 M Ba(OH)₂. What is the concentration…

A: Balanced chemical equation: 2HCl + Ba(OH)2 -------> BaCl2 + 2H2O So, Number of moles of…

Q: An aqueous solution of a strong monoprotic acid (HA) contains 0.550 g of acid and is completely…

A: Titration The molar mass of a compound can calculate using its given mass and the number of moles.…

Q: The identity of an unknown monoprotic organic acid is determined by titration. A 0.701 g sample of…

A: Answer:- Given data:- mass of sample = 0.701 g molarity of NaOH…

Q: A 25.0 mL solution of HBr is neutralized with 13.6 mL of 0.105 M Sr(OH)₂. What is the concentration…

A: Given , M2 = 0.105 M V1 = 25.0 ml V2= 13.6 ml M1 = ?

Q: Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows. Zn(s) + 2HCl(aq) → ZnCl2(aq)…

A: The balanced reaction taking place is given as, => Zn (s) + 2 HCl (aq) ----------> ZnCl2 (aq)…

Q: A 15.00 mL solution of phosphoric acid (H3PO) is titrated with 11.20 mL of 0.155 M sodium hydroxide.…

A: Given data: Volume of acid = 15 mL Volume of base = 11.20 mL Molarity of base = 0.155 M Formula…

Q: Instead of using ratios for back titrations we can also use molarities, if our solutions are…

A: Step 1: First of all, the moles of Al(OH)3 is obtained from the given data. But, here the data is…

Q: Zn(s)+ 2 HCl(aq)®ZnCl2(aq)+ H2(g). What mass of hydrogen gas is produced when a 7.35 g chunk of…

A: Moles of zinc reacting = mass of zinc / Atomic mass of zinc => moles of Zn = 7.35 / 65.4 =…

Question

20 g a sample of Ba(OH)2 is dissolved in 10 mL
of 0.5 N HCL solution: The excess of HCL was
titrated with 0.2 N NaOH. The volume of
NaOH used was 20 cc. Calculate the
percentage of Ba(OH)2 in the sample.

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 1

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

An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.
The equivalence point for the titration of a 25.00-mL sample of CSOH solution with 0.1062 M HNO3 is at 35.27 mL. What is the concentration of the CsOH solution?
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
What acid-base indicators, shown in Figure 18.24 would be suitable for the neutralization reaction whose titration curve is shown in Figure 18.30?Why?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
8-98 When a solution prepared by dissolving 4.00 g of an unknown monoprotic acid in 1.00 L of water is titrated with 0.600 M NaOH, 38.7 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown acid?
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?