NaHCO, can be used to neutralize excess acid in situations such as, for instance, acid spills in the laboratory. The reaction is: H'(ag) = HCO3 (aq) H2O(1) + CO2(g). How many grams of NaHCO3 would be required to neutralize the acid in 75.5 mL of 1.00 M nitric acid? O 6.34 grams O 75.5 grams O 0.899 grams O 1.11 grams O 7.55 grams eTextbook and Media Attempts: 0 of 2 used Submit Answer Save for Later

NaHCO, can be used to neutralize excess acid in situations such as, for instance, acid spills in the laboratory. The reaction is: H'(ag) = HCO3 (aq) H2O(1) + CO2(g). How many grams of NaHCO3 would be required to neutralize the acid in 75.5 mL of 1.00 M nitric acid? O 6.34 grams O 75.5 grams O 0.899 grams O 1.11 grams O 7.55 grams eTextbook and Media Attempts: 0 of 2 used Submit Answer Save for Later

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Al(NO3)3(aq) + 3K3PO4(aq) ⟶ AlPO4(s) + 9KNO3(aq) What is the maximum mass of aluminum phosphate that will precipitatefrom a solution prepared by adding an excess of an Al(NO3)3 solution to50.00 mL of 1.525 M K3PO4?
F12 F11 ID: A Date: Class: ID: A 24. 6. The amount of calcium present in milk can be determined by adding oxalate to a sample and measuring the mass of calcium oxalate precipitated. What is the mass percent of calcium if 0.429 g of calcium oxalate forms in a 125-g sample of milk when excess aqueous sodium oxalate is added? Na,C2O4(aq) + Ca²*(aq) → CaC2O4(s) + 2Na*(aq) a. 0.107% b. 0.202% с. 0.343% d. 1.10% е. 1.37% 25. Identify all the spectator ions in the following reaction. KSO4(aq) + 2MNSO4(aq) + 5FE2(SO4)3(aq)
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCI(aq) + MnO,(s) → MnCl, (aq) +2 H,O(1) + Cl, (g) A sample of 35.5 g MnO, is added to a solution containing 50.9 g HCI. What is the limiting reactant? HCI O MnO, What is the theoretical yield of CI,? theoretical yield: g Cl, If the yield of the reaction is 86.3%, what is the actual yield of chlorine? actual yield: g Cl,
Ff.141.
Balance the following chemical equations (type corresponding coefficients (1, 2, 3, ...) in blanks). NO2 + F2→ NO2F
A sample of soda ash (impure Na2CO3) is titrated with 0.5000 N H2SO4. If the sample weighs 1.1000 g and requires 35.00 mL of the acid for complete neutralization, what is the %Na2CO3 in the ash assuming no other active component is present?
15. If 23.0 mL of a 1.00 M Ba(NO3)2 solution was reacted with 55.0 mL of a 0.700 M solution of K3PO4 to produce the solid Ba3(PO4)2 by the balanced chemical equation 3 Ba(NO3)2 (aq) + 2 K3PO4(aq) – Ba3(PO4)2(s) + 6 KNO3(aq) a. What is the limiting reagent? AS b. How many grams of Ba3(PO4)2 will be produced? elomibt.ESE -3HA
In the following reaction, 35.0 mL of 0.150 M magnesium bromide solution reacts with excess silver nitrate to form a precipitate. What is the expected mass of AgBr in grams? (molar mass of AgBr = 187.77 g/mole) MgBr2(aq) + 2AgNO3(aq) --> 2AgBr(s) + Mg(NO3)2(aq) Question 11 options: 0.985 g 0.493 g 1.97 g 986 g none of these
If a solution containing 58 g of mercury(II) nitrate is allowed to react completely with a solution containing 16.642 g of sodium sulfate according to the equation below: Hg(NO3)2(aq)+Na2SO4(aq)------2NaNO3(aq)+HgSO4(s) A. How many grams of solid precipitate will be formed if the reaction has a 100% yield? B. How many grams of the excess reagent will remain after the reaction? C. If the reaction has only an 80% yield, how many grams of solid precipitate will be formed?
Consider the following reaction: (reaction in image), what mass of AI2(SO4)3 will be produced from 355 mL of 0.200 M H2SO4 solution? ___ g (provide answer to correct sig figs in units of g)
Fumaric acid is quite common in the plant world and is added to many foods due to its acidity and fruity flavor. It has a molar mass of 116.07 g/mol and a formula of C4H4O4. A solution of sodium hydroxide is used to determine the molarity of a fumaric acid acid solution before it is used to prepare some sour gummi worms. C4H4O4(aq) + 2NaOH(aq) --> Na2C4H2O4(aq) +2 H2O(l) Calculate the Molarity of the fumaric acid if 32.08 mL of 0.09973 M NaOH was used to neutralized 75.00 mL of fumaric acid solution. Assume the fumaric acid is acting as a strong electrolyte acid in this reaction. (It is a weak acid, but a very strong weak electrolyte) Fumaric acid is quite common in the plant world and is added to many foods due to its acidity and fruity flavor. It has a molar mass of 116.07 g/mol and a formula of C4H4O4. A solution of sodium hydroxide is used to determine the molarity of a fumaric acid acid solution before it is used to prepare some sour gummi worms.…