A mass of 3.3214 g of sodium bi carbonate was dissolved and and diluted to 250,00 ml of aqueous solution .A 20.550X mL of sodium bicarbonate was used to neutralise 25.00mL of H2SO4solution. Calculate the molar concentration of H2SO4 SOLUTION

A mass of 3.3214 g of sodium bi carbonate was dissolved and and diluted to 250,00 ml of aqueous solution .A 20.550X mL of sodium bicarbonate was used to neutralise 25.00mL of H2SO4solution. Calculate the molar concentration of H2SO4 SOLUTION

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 solution of phthalic acid was titrated to a pH of 4.63. a. What are the 2 main species present in…

Q: Calculate the mass percent of acetic acid, HC,H,0,(aq), in the vinegar using the molar con-…

A: using the molarity formula we can calculate the molarity and vinegar have a 4.3% acetic acid…

Q: The solubility (denoted as s) of CaSO4 in pure water at 40o C is 1.09 grams per liter. What is the…

Q: what mass of solid lanthanum oxalate nonahydrate can be obtained from 650 ml of 0.0170 m aqueous…

Q: 73.33.5ml of 0.9998N NaOH was used in the titration of 50m! HCI solution. Calculate the normality. 3

A: In this question, we will determine the normality of HCl. You can see the details calculation…

Q: 1.11 M hydrazine, N2H4(aq). (Kp = 1.3 x 106). pH = i Save for Later

Q: The solubility of nitrogen gas at 20 C is 19 mg/L. Calculate the maximum molar and mass…

Q: Given that 1ml of 0.01M AgNO3 =0.35mg of Clion calculate the concentration of Cl ion per ml of the…

Q: Discuss what is present in the resulting solution when 15.0 mL of 0.1 M HCl is added to 15.0 mL of…

A: The balanced chemical equation will be: HCl + NaOH ---------------------------> NaCl + H2O

Q: A sample consisting of an aqueous solution of the monoprotic acetic acid (CH3COOH, 60.05g/mol) is…

A: Molarity of NaOH given = 0.2024 M Volume of NaOH used to reach end point = 22.67 mL Wt. of Acetic…

Q: A 10.00 mL sample of vinegar is titrated with 0.265M NaOH and requires 25.90mL of NaOH to reach the…

A: Vinegar is made of acetic acid and water.

Q: The temperature for each solution is carried out at approximately 297 K where K w =1.00×10 −14 0.85…

A: Given, Kw = 1.00*10-14. Mass of HCl = 0.85g. Volume of solution = 5.5L. Moles and molarity of HCl…

Q: what volume of water should be added to 1.0dm^3 of 0.5M AgNO3 to adjust the concentration to 125mM?

A: s Given initial concentration is 0.5M in 1 dm3 Since, 1 dm3 = 1L Therefore, concentration is 0.5M in…

Q: Citric acid, H3C6H5O7, is an example of a triprotic acid. A solution of citric acid is extracted…

Q: A tablet contains 0.5 g of magnesium hydroxide as the only basic ingredient . The tablet is analysed…

Q: With the help of a schematic diagram representing the titration of samples contanining various forms…

Q: The normal boiling point of water, H20 is 100.00 °C and its Kpp value is 0.512 °C/m. Assuming…

A: Given: Mass of Fe(CH3COO)3 = 13.32 g. Mass of water i.e. solvent = 273.4 g = 0.2734 Kg…

Q: 136 mL of 0.00015 M Pb(NO3)2 and 234 mL of 0.00028 M Na2SO4 (volumes are additive). Will a…

Q: Calculate the concentration of sodium jons in solution after 30.0 mL of 3.35 M NaCI and 70.0 mL of…

Q: a) What is the molar concentration of the Solution in 250.0mL b) if loo.OmL of solvent is added to…

A: Mass of AuCl3 = 53.3g Volume of water = 250mL

Q: Suppose, in an experiment to determine the amount of sodium hypochlorite in bleach, you titrated a…

A: Given data,Molarity of KIO3=0.010MVolume of KIO3=26.34mLVolume of Na2S2O3=15.51mL

Q: Iness is 250 mg/l as CaCO2 and alkalinity is 150 mg/1 as CaCO3.

A: Total hardess of water is the sum of carbonate and non carbonate hardness in term of mg/L as CaCO3.…

Q: How many millilitersof a 0.452M Na2Osolution is required to completely precipitate allthe aluminumin…

A: Given: Concentration of Na2O = 0.452M Concentration of Al(NO3)3 solution= 0.355M Volume of…

Q: If we mix 17.1mL of 0.100M Lil, 20.7mL of 0.100M Cal2 and 27.3mL of 0.100M Li2SO4, what will be the…

Q: A solution of 1.7×10−6 M HNO3(aq) (10.0 mL) is diluted to 10.0 L with pure deionized water at 25 °C…

Q: A 5.00 mL solution of H,SO4 was transferred to a 25.00 mL volumetric flask and was diluted to the…

Q: A saturated solution of lead(II) sulfate can be prepared by diluting 0.0183 g of PbSO4 (MM= 303.26…

A: We have to find the Ksp of PbSO4

Q: The sôlution of known concentration is called Original Solution O A. Indicator OB. Buffer Solution…

A: A standard solution : standard solution is a solution containing a precisely known concentration of…

Q: The acidic water of a lake (V = 4 x 108 L) must be neutralized with lime, Cao. It will require a…

A: Initial pH of the lake = 5.6 Thus, initial [H+] is determined as- [H+]=10-pH =10-5.6∴[H+]=…

Q: If you were provided with 250mL of 0.25M solution of CuSO4 explain the effect of the overall…

Q: molarity

Q: Describe how you would prepare a) 7.00L of 0.0500M potassium permanganate solution from solid…

A: a) Given that - Volume of KMnO4 Solution = 7.00 L = 7000 mL Molarity of solution = 0.0500 M…

Q: The problem with making a standard solution of sodium hydroxide from solid NaOH is that O a. the…

A: NaOH is a commonly used laboratory agent. The solution of standard NaOH can be prepared using…

Q: Estimate the carbon dioxide content ui a natural water sample having a pH of 7.3 and a…

A: The value of Ka is standard so is taken from book. [H+] and [H3O+] are one and the same thing…

Q: A 0.250 g sample of the weak acid HA (molar mass = 150.0 g/mol) is dissolved in 50.0 g of water. The…

Q: Suppose 25.0 g of solid NaOH is added to 1.50 L of anaqueous solution that is already 2.40 M in…

Q: Calculate the solubility, in milligrams, of MGF2 (MM = 62.31g/mol) in 100. mL of 0.10 M NaF(aq)…

A: Given : Ksp = 3.7 x 10-8

Q: The concentration of an aqueous solution of CaSO4 (Ksp = 7.1 × 10–5) is 8.43 × 10–3 M. Qsp = ___ and…

A: Ksp stand for solubility product. Qsp stands for Solubility Product Quotient and is used to…

Q: A 30.0 mL sample of this aqueous HX solution freezes at – 0.186 oC. A. What is the molal…

A: Since you have asked multiple questions, we shall answer only one. Please ask the questions…

Q: Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000552 mol…

Q: Problem attached

A: Density of a compound is calculated by dividing mass of the compound with the volume of the…

Q: A solution of 20 ml of 1O N KOH required 20.3 ml of NaOH solution when end point of Titration was…

Q: A 5.00 mL sample of drinking water contains 15% by weight CI, was titrated with 0.1M AgNO3 using…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: A mass of 3.3214 g of sodium bicarbonate was dissolved and diluted to 250.00 ml of aqueous solution.…

Q: A 0.001 m solution of a weak electrolyte ionizes into 4 ions freezes at -0.06C. What is the apparent…

A: Given: Molality of weak electrolyte = 0.001 m And the freezing point of the solution = -0.06 oC

Q: Vhat is the caustic alkalinity of a solution with a carbonate concentration of 20 ng/L and a pH of…

A: Given- 100 ml from water , pH = 8.1 '

Q: Balanced Chemical Equation NaOH + HA-> NaA + H2O Details Volume (mL) of original unkown acid (HA)…

A: The balanced titration equation is: NaOH + HA → NaA + H2O

Concept explainers

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.

Question

A mass of 3.3214 g of sodium bi carbonate was dissolved and and diluted to 250,00 ml of aqueous solution .A 20.550X mL of sodium bicarbonate was used to neutralise 25.00mL of H₂SO₄solution. Calculate the molar concentration of H₂SO₄SOLUTION

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps

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

When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.
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?
Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?
A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Distinguish between the terms slightly soluble and weak. electrolyte.
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?