Question

A 0.40 gram sample of NaOH (molar mass = 40.0 g/mol) was completely neutralized with 62.5...

A 0.40 gram sample of NaOH (molar mass = 40.0 g/mol) was completely neutralized with 62.5 mL of H2SO4 solution. Assume the chemical equation is: H2SO4(aq) + 2NaOH(aq)  Na2SO4(aq) + 2H2O(l). What is the molarity of the H2SO4 solution?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Given Reaction

H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l).

Step 1: From the given reaction, It is noted that 2 mole of NaOH require 1 mole of Sulfuric Acid

Step 2: We have to find out mole of NaOH for the given amount(Weight)

i.e., 40g of NaOH = 1M[NaOH]   

Therefore, 0.4g of NaOH= 0.01 M[NaOH]   

Step 3: From the given reaction

For 2M of NaOH, 1M of H2SO4 is required. Therefore 0.01 M of NaOH requires 0.005M of H2SO4

Ans: Molarity of the 62.5 mL  H2SO4 solution =  0.005M

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
33. When 45.0 g NaOH and 40.0 g H2SO4 are mixed and reacted, which is the...
33. When 45.0 g NaOH and 40.0 g H2SO4 are mixed and reacted, which is the limiting reagent? H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)
100.0 mL of 0.800 M aqueous NaOH and 50.00 mL of 0.800 M aqueous H2SO4, each...
100.0 mL of 0.800 M aqueous NaOH and 50.00 mL of 0.800 M aqueous H2SO4, each at 24.0°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 29.3 °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 a specific heat capacity of 4.18 J/(g•K).     How much heat was absorbed by the water?
In an experiment, 25.0 mL of 0.145 M H2SO4 react completely with 54.1 mL of a...
In an experiment, 25.0 mL of 0.145 M H2SO4 react completely with 54.1 mL of a NaOH solution. What is the molar concentration (M) of the NaOH solution? 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O a. 2.52 M b. 0.134 M c. 0.323 M d. 1.67 M e. 0.250 M Please show work! Thanks
Calculate the mass of KHC8H4O4 (molar mass = 204.23 g/mol) that reacts with 25.0 mL of...
Calculate the mass of KHC8H4O4 (molar mass = 204.23 g/mol) that reacts with 25.0 mL of 0.150 M NaOH solution. KHC8H4O4(aq) + NaOH(aq) → H2O(l) + NaKC8H4O4(aq) a)0.383 g b)0.766 g c)1.88 g d)1.53 g e)3.75 g
1.Percent by mass to parts per million. Convert 4.45% NaOH(aq) solution to parts per million NaOH...
1.Percent by mass to parts per million. Convert 4.45% NaOH(aq) solution to parts per million NaOH in the solution. Do NOT assume a dilute aqueous solution! Use the molar mass of the entire salt formula, not either ion alone. The solution density is 1.047 g/mL. Answer to 3 significant figures with appropriate units. 2. Molarity to parts per million. Convert 1.672 mol/L MgCl2(aq) solution to parts per million Mg2+ in the solution. Do NOT assume this is a dilute aqueous...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution...
Based off info below please answer blank boxes. Thanks! Application Questions: 12. Before using a solution of NaOH as a standard for a titration, its precise concentration must be determined by titration with a standard acid. This is because solid NaOH absorbs water from the atmosphere, so its solid form is difficult to keep free of contaminated H2O. A common acid used for standardization is the acid-salt, potassium hydrogen phthalate (KHP), KHC8H4O4. Another way is to use a standardized solution...
A 36.0mL sample of aqueous sulfuric acid was titrated with 0.250 molar KOH (aq) until the...
A 36.0mL sample of aqueous sulfuric acid was titrated with 0.250 molar KOH (aq) until the chemical indicator signaled that the solution was exactly neutralized. The mixture was then carefully evaporated to dryness, then the residue was dried in a drying oven. The residue was then weighed and a value of 861 my was obtained for it's mass. Calculate the number of mL of the potassium hydroxide solution that was used in the titration from this data. H2SO4 + 2KOH...
26. You are provided with a 250 mL volumetric flask, deionized water and solid NaOH. a)...
26. You are provided with a 250 mL volumetric flask, deionized water and solid NaOH. a) How much NaOH should be weighed out in order to make 250. mL of 0.100 M solution? (5points) b) You have deionized water, the mass of sodium hydroxide found in part a and the volumetric flask. In what order and how much of the two substances, water and NaOH, do you add to the flask? ( 4 points) i) First you add _______________ (amount)...
A 0.616 gram sample of a metal, M, reacts completely with sulfuric acid according to: M(s)...
A 0.616 gram sample of a metal, M, reacts completely with sulfuric acid according to: M(s) + H2SO4(aq) ------> MSO4(aq) +H2(g) A volume of 239 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr and the temperature is 25 °C. Calculate the molar mass of the metal.
A 0.4126 g sample of primary-standard Na2CO3 was treated with 40.0 mL of diluted perchloric acid....
A 0.4126 g sample of primary-standard Na2CO3 was treated with 40.0 mL of diluted perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back titrated with 9.20 mL of dilute NaOH. In a separate experiment, it was stablished that 22.93 mL of the HClO4 neutralized the NaOH in a 25.00 mL portion. Calculate the molarity of the HClO4 and NaOH. Please report correct Significant Figures and explain
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT