Automobile batteries use 3.0 M H2SO4 as an electrolyte. How much 2.40 M NaOH will be...
Automobile batteries use 3.0 M H2SO4 as an electrolyte. How much 2.40 M NaOH will be needed to neutralize 165.7 mL of battery acid? H2SO4(aq) + 2NaOH(aq) → 2H2O(l) + Na2SO4(aq) Round off to 2 significant figures. Do not include unit, L. Do not use scientific notation.
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Automobile batteries use 3.0 M H2SO4 as an electrolyte. How much
2.40 M NaOH will be...
A solution of 0.154 M NaOH is used to neutralize 25.5 mL of a H2SO4 solution....
A solution of 0.154 M NaOH is used to neutralize 25.5 mL of a H2SO4 solution. If 25.0 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution? H2SO4(aq)+2NaOH(aq)→2H2O(l)+Na2SO4(aq)
How many milliliters of 0.100 M NaOH are required to neutralize 65.0 mL of 0.250 M...
How many milliliters of 0.100 M NaOH are required to neutralize 65.0 mL of 0.250 M H2SO4 ? The balanced neutralization reaction is: H2SO4(aq)+2NaOH(aq)→Na2SO4(aq)+2H2O(l).
1.What is the final concentration of a solution of KCl that is prepared by adding 46mL...
1.What is the final concentration of a solution of KCl that is prepared by adding 46mL of a 2.98M KCl solution to a flask for a final volume of 245 mL? 2.What volume( in mL) of a 1.89M solution of NaF is needed to prepare 406mL of a 0.35M solution of NaF? 3.Calculate the mass of Al metal needed to react with 87 mL of a 3.18M solution of HNO3. Al(s) + HNO3(aq) --> Al(NO3)3 + H2(g) ( unbalanced) 4.Calculate...
How many milliliters of 0.250 M NaOH are required to neutralize 55.0 mL of 0.300 M H2SO4?
How many milliliters of 0.250 M NaOH are required to neutralize 55.0 mL of 0.300 M H2SO4? The balanced neutralization reaction is: H2SO4(aq) +2 NaOH(aq) → Na2SO4(aq)+2H2O(l).
Consider the reaction H2SO4(aq) + 2NaOH(aq) → 2H2O(l) +Na2SO4(aq). If 25 mL of H2SO4 was needed to react with 15 mL of 0.20 M NaOH, what is the molarity of the H2SO4(aq)?
Consider the reaction H2SO4(aq) + 2NaOH(aq) → 2H2O(l) +Na2SO4(aq). If 25 mL of H2SO4 was needed to react with 15 mL of 0.20 M NaOH, what is the molarity of the H2SO4(aq)?
25.00 mL of a sulfuric acid solution was standardized by titration with 0.2500 M NaOH using...
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...
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...
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each...
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each at 24.00°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 26.65 °C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1.00 g/mL and specific heat capacity of 4.18 J/(g•C) How much heat did the reaction release?
In a titration, 23.57 mL of 1.37 M NaOH were added to an acid. How many...
In a titration, 23.57 mL of 1.37 M NaOH were added to an acid. How many moles of NaOH were added? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific notation. In a titration, 50.00 mL of 0.916 M H2SO4 were added. How many moles of H* were delivered? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific...
What volume of 0.259 M H2SO4 is needed to react with 60.0 mL of 0.112 M...
What volume of 0.259 M H2SO4 is needed to react with 60.0 mL of 0.112 M NaOH? The equation is H2SO4(aq) + 2NaOH(aq)Na2SO4(aq) + 2H2O(1) ΑΣΦ PI ? VH2SO4 = mL Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
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...
In a titration, 23.57 mL of 1.37 M NaOH were added to an acid. How many moles of NaOH were added? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific notation. In a titration, 50.00 mL of 0.916 M H2SO4 were added. How many moles of H* were delivered? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific...
What volume of 0.259 M H2SO4 is needed to react with 60.0 mL of 0.112 M NaOH? The equation is H2SO4(aq) + 2NaOH(aq)Na2SO4(aq) + 2H2O(1) ΑΣΦ PI ? VH2SO4 = mL Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
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