A 25.00 mL sample of an unknown sulfuric acid solution is titrated with 29.84 mL of...
m Stoichiometry #2 At Home Practice • Show all work using the factor label method • Use units and label chemical formulas for all conversion factors • Report final answer with the correct number of slunificant figures, unit and chemical formula What volume, in L of 0.250 MKCI will completely react with 0.175 L of a 0.225 M Pb(NO,h solution based upon the following equation rrrrrrrr 2 KCl(aq) + Pb(NO3)(aq) → PbCI:(s) + 2 KNO3(aq) Show your work Final Answer...
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation H2SO4 + 2NaOH + 2H2O + Na2SO4 If you require 28.52 mL of 0.904 M NaOH solution to titrate 209.1 mL of H2SO4 solution, what is the concentration of the H2SO4 solution? Type answer:
25.00 mL of a sulfuric acid solution was standardized by titration with 0.2500 M NaOH using phenolpthalein indicator. 30.52 ml of the NaOH was required. Find the molarity of the sulfuric acid. H2SO4 (aq) + 2NaOH (aq) ----> Na2SO4 (aq) + 2H2O (l)
1) A flask containing 450.0 mL of 0.500 M HBr was spilled on the floor. How many grams of K2CO3 would you need to put on the spill to neutralize the acid according to the following reaction? 2 HBr (aq) + K2CO3 (s) => 2KBr (aq) + H2O (l) 2) Determine the molarity of an unknown NaOH solution if 25.00 mL of sodium hydroxide was titrated with 15.00 mL of a 1.500 M sulfiric acid solution (H2SO4). (aOH= 40.00 g/mol...
An unknown sample of sulfuric acid was determined by the method used in this experiment. The sodium hydroxide was standardized by titration of 0.0855g of oxalic acid dihydrate with 25.28mL of sodium hydroxide. 10.00ml of the unknown sulfuric acid was then titrated to endpoint with 32.34mL of the same sodium hydroxide solution. What was the concentration of the sulfuric acid? (Show your work!!)
If 32.12 mL of 3.77 M hydrochloric acid solution, HCl, are titrated with 51.5 mL of sodium hydroxide solution, NaOH, according to HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) what is the concentration of the sodium hydroxide solution? (Enter your
A student titrated a 25.00-mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of 0.1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample. (a) 9.184 x 10‒4 M (b) 3.674 x 10‒2 M (c) 7.304 x 10‒2 M (d) 7.347 x 10‒2 M (e) 1.469 x 10‒1 M
Sulfuric acid (250.0 mL) is titrated with 176.5 mL 2.4 M NaOH to an equivalence point (the point where all the sulfuric acid is exactly neutralized). 2 NaOH + H2SO4 → 2 H2O + Na2SO4 (a) How many moles of sulfuric acid were in the original 250.0 mL? (b) What was the concentration of sulfuric acid in the original 250.0 mL sample?
A 25.00 mL solution of H2SO4 of unknown concentration was titrated with a 3.15 M NaOH solution. What is the concentration of the H2SO4 solution if 36.01 mL of the NaOH solution is required neutralize the acid solution?
you are asked to tittate a sample of sulfuric acid of unknown concentration against a standardized solution if sodium hydroxide. you stsrt with 23.00 mL of sulfuric acid in a reaction flask, and 25.67 mL of 1.760 M sodium hydroxide are required to reach the equivalent point, what is the molarity (M) of the sulfuric acid solution? please show conversion steps!