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Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution...
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid of unknown concentration with a standardized base. At the beginning of the titration, you read the base titrant volume as 2.86 mL. After running the titration and reaching the endpoint, you read the base titrant volume as 21.17 mL. What volume, in mL, of base was required for the titration? Type answer: Question 6 Status: Not yet answered Points possible: 1.00 Suppose you are...
Sodium hydroxide reacts with sulfuric acid according to the equation 2NaOH (aq) + H2SO4 (aq) -----> Na2SO4 (aq) + 2H2O (l) Suppose that a solution containing 60.0 grams of sodium hydroxide is added to one containing 20.0 grams of sulfuric acid. How many grams of sodium sulfate will be produced?
Considering the titration of sulfuric acid with sodium hydroxide, what is the balanced neutralization equation? O NaOH + 2H2SO4 -> H2O + 2Na2504 O 2NaOH + H2SO4 -> 2H2O + Na2504 O NaOH + H2SO4 --> H2O + Na2SO4 O 2NaOH + H2504 --> H2O + Nas04
A 25.00 mL sample of an unknown sulfuric acid solution is titrated with 29.84 mL of a sodium hydroxide solution with a concentration of 0.150 M NaOH. What is the concentration of the sulfuric acid solution? H.SO.(aq) + 2NaOH(aq) → Na2SO4 (aq) + 2 H2O(1) Show your work Final 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...
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!
You need to neutralize a solution of an unknown concentration of sodium hydroxide before you can dispose of it. In the lab, you have a 5.0M bottle of hydrochloric acid, however, you want to dilute that first to use a less concentrated (and less dangerous) solution. So, you decide to use a 0.1M solution of hydrochloric acid solution and to make 2.0 litres of it. (a) Show all calculations for how you would do this. (b) Once you have your...
3. Sodium hydroxide (NaOH) reacts with sulfuric acid (H2SO4) to yield sodium sulface (Na2SO4) and water (H2O). The equation for the reaction is wNaOH + H2SO4 →yNa2SO4 + 2H2O, where w, x, y, and z must be chosen to balance the equation. (a) Translate the chemical equation into a system of four linear equations, where each equation balances the number of atoms of a particular element. (b) Express the system as an augmented matrix and solve by Gauss-Jordan elimination. (c)...
Given the following equation, calculate the amount of sodium hydroxide (in moles) required to react with 26.1 mol sulfuric acid to exactly neutralize it. 2NaOH + H2SO4 --> 2H2O + Na2SO4