A 1.18 M solution of citric acid (H3C6H507, MW=192.122 g/mol) in water has a density of...
A solution of NaCl (MW = 58.5 g/mol) in water (MW = 18.0 g/mol) has the molality of 3.01 molal and the density of 1.112 g/mL. Consider mass of solvent 1 Kg A) What is the mass percent of the solute? (B) What is the molarity of the solution? (C)What is the mole fraction of H2O?
An aqueous solution is 36.0° by mass hydrochloric acid, HCl, and has a density of 1.18 g ml. The molarity of hydrochloric acid in the solution is M Subrnit Answer Try Another Version 1 item attempt remaining
Consider a different analyte for this exercise. Citric acid is found in many fruits and fruit juices. Sodium hydroxide (NaOH) is the titrant and citric acid (H2C6H507) the analyte according to the following balanced chemical equation. H3C6H507 + 3OH- → C6H50,3- + 3 H20 (a) What is the stoichiometry of H3C6H507 to OH ? UN OOOOOOO (b) Complete the following table for this titration. Data Table P2: Titration of citric acid in orange juice with sodium hydroxide. concentration of OH-...
B. Commercial nitric acid comes in a concentration of 16.0 mol/L. The density of this solution is 1.42 g/mL Calculate the percent (w/w) of nitric acid, HNO3, in this solution. How many milliliters of the concentrated acid have to be taken to prepared 250 g of a solution that is 10.0%(w/w) HNO3? C. Citric acid, H3C6H5O7, occurs in plants. Lemons contain 5% to 8% citric acid by mass. The acid is added to beverages and candy. An aqueous solution...
A 1.00-9 solid sample containing a mixture of table salt (NaCl) and citric acid (H3C6H507, a triprotic acid) is dissolved in 15 mL of water. Titration of the acid solution requires 17.70 mL of 0.5602 M NaOH solution to reach the endpoint. Calculate the mass percent H3C6H5O7 in the solid mixture. (Number only) %
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water to produce a 50.0 mL solution. The pH of this solution is measure to be pH = 2.13. Determine the ionization constant (Ka) of the acid. 8. A buffer is 0.50 M CH3COOH(aq) and 0.50 M Na(C6H-C00) (aq). For CH2COOH pKa = 4.20 a) Calculate the pH of the buffer solution. b) Calculate the pH after the addition of 40 mL of a 0.150...
A concentrated HNO3 (MW = 63.0128 g/mol) solution is 70.0 %wt HNO3 and has a density of 1.42 g/mL. How many milliliters of the concentrated HNO3 solution must be diluted to obtain 500.0 mL of 1.00 M HNO3?
A 100.0 mL100.0 mL solution containing 0.927 g0.927 g of maleic acid (MW=116.072 g/mol)(MW=116.072 g/mol) is titrated with 0.275 M KOH.0.275 M KOH. Calculate the pH of the solution after the addition of 58.0 mL58.0 mL of the KOHKOH solution. Maleic acid has p?apKa values of 1.92 and 6.27. pH= At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated as H2M,H2M, HM−,HM−, and M2−,M2−,...
The combustion of C17H36 (Mw = 240. g/mol) results in the formation of water and carbon dioxide. How many grams of carbon dioxide (Mw = 44.g/mol) are produced when 50,4 g of C17H36 burns? _C17H36+ - 02__CO2+ H₂O 1.6x10²8 3.570 3.6 None of these choices are correct.
5.3307 g of Na2CrO4 (MW 161.97 g/mol) is dissolved in 1000.0 mL of water. Assuming the solution has a density of 1.00 g/mL, what is the concentration of Na (MW 22.9898 g/mol) in the solution in units of a) molarity (M)? Number b) parts per thousand (ppt)? Number ppt c) 25.0 mL of the solution is then diluted to a final volume of 500.0 mL. What is the concentration of Na* in the diluted solution in units of parts per...