85ml of 0.1M H_2SO_4 solution is titrated against 0.1N KOH solution. Calculate the concentration...
Question:
85 mL of 0.10 M {eq}\rm H_2SO_4 {/eq} solution is titrated against 0.10 N KOH solution. Calculate the concentration of salt formed when the acid is one fourth neutralized.
Neutralization Reaction:
A neutralization reaction is when an acid and base are mixed in chemically equivalent quantities to reach the required equivalence point. For a diprotic acid titrated with a Group 1 alkali metal hydroxide base, this will require a 1:2 molar ratio to reach the equivalence point. This neutralization reaction will form water and a salt as products.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThis neutralization reaction will produce potassium sulfate as a salt:
{eq}\rm H_2SO_4 (aq) + 2KOH (aq) \rightarrow 2H_2O (l) + K_2SO_4 (aq) {/eq}
- m...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Neutralization and Acid-Base Reactions
from
Chapter 10 / Lesson 5
37K
Learn about acid-base neutralization reactions. Understand the reaction between acid and base, the neutralization reaction, the definition, and see the products.
Related to this Question
- Sulfuric acid, H_2SO_4, can be neutralized with a solution of potassium hydroxide, KOH. a. Write a chemical equation for this neutralization reaction? b. 20.00 mL of an H_2SO_4 solution of unknown concentration was titrated to an endpoint with 0.1368
- It takes 56 mL of 0.124 M KOH to neutralize 45.4 mL of H_2SO_4 solution. What is the concentration of the H_2SO_4 solution?
- It takes 75 mL of 0.124 M KOH to neutralize 28.5 mL of H_2SO_4 solution. What is the concentration of the H_2SO_4 solution?
- It takes 62 mL of 0.124 M KOH to neutralize 46.7 mL of H_2SO_4 solution. What is the concentration of the H_2SO_4 solution?
- A 15.0 mL of 0.174 M H_2SO_4 is neutralized by 18.1 mL of KOH solution. The molarity of the KOH solution is:
- Determine the volume of 0.250 M KOH solution required to neutralize 205 mL of 0.130 M H2SO4 sulfuric acid. The neutralization reaction is: H2SO4(aq) + 2KOH(aq) = K2SO4(aq) + 2H2O(l)
- If it takes 50.0 mL of a 0.5 M KOH solution to completely neutralize 125.0 mL of a sulfuric acid solution, what is the concentration of the sulfuric acid solution?
- If it takes 50.0 mL of a 0.75 M KOH solution to completely neutralize 150.0 mL of a sulfuric acid solution, what is the concentration of the sulfuric acid solution?
- Determine the volume of 0.220 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H_2SO_4(aq) + 2KOH(aq) \to K_2SO_4(aq) + 2H_2O(l) a) 55 mL of 0.115 M H_2SO_4 b) 165 mL of 0.135 M H_2SO_4
- Determine the volume of 0.240 M KOH solution required to neutralize 25 mL of 0.240 M H2SO4 solution.
- Determine the volume of 0.240 M KOH solution required to neutralize 155 mL of 0.140 M H2SO4 solution.
- Determine the volume of 0.240 M KOH solution required to neutralize 70 mL of 0.120 M H2SO4 solution.
- Determine the volume of 0.250 M KOH solution required to neutralize 15 mL of 0.250 M H2SO4. The neutralization reaction is: H2SO4(aq) + 2KOH(aq) = K2SO4(aq) + 2H2O(l)
- It takes 62 mL of 0.124 M KOH to neutralize 46.7 mL of H_2SO_4 solution. What is the concentration of the H_2SO_4 solution? Answer in units of moles/liter
- Calculate the volume of KOH needed to completely titrate 25.00 ml of a 0.1550 M solution of sulfuric acid if the concentration of potassium hydroxide was 0.2174 M.
- We find that 18.90 mL of a 2.50 M KOH solution is required to titrate 35.0 mL of an H2SO4 solution. What is the molarity of the H2SO4 solution?
- For the following reaction: H_2SO_4 + 2KOH to 2 H_2O + K_2SO_4 If 38.2 mL of 0.163 M KOH is required to neutralize completely 25.0 mL of a H_2SO_4 solution, what is the molarity of the acid?
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aq. solution. 0.350 L of 0.410 M H_2SO_4 is mixed with 0.300 L of 0.230 M KOH. What concentration of sulfuric acid remains after n
- 1) Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution. 2) 0.650 L of 0.400 M H_2SO_4 is mixed with 0.600 L of 0.250 M KOH. What concentration of sulfuric acid remai
- If 37.8 mL of a 0.160 M KOH solution is required to titrate 28.5 mL of a H_2SO_4 solution, what is the molarity of the H_2SO_4 solution? H_2SO_4(aq)+2KOH(aq)\to 2H_2O(l)+K_2SO_4(aq)
- A 25.00 mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 43.22 mL of KOH is required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? Express your answer
- Suppose 10.0 mL of a 0.121 M H2SO4 solution is neutralized by 17.1 mL of a KOH solution. What is the molarity of the KOH solution?
- A 29.00 mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1122 M KOH solution. A volume of 43.22 mL of KOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? (Express your answe
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution. Phases are optional. 0.850 L of 0.460 M H_2SO_4 is mixed with 0.800 L of 0.200 M KOH. What concentration of sul
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution. Phases are optional. 0.950 L of 0.440 M H_2SO_4 is mixed with 0.900 L of 0.280 M KOH. What concentration of su
- A 15.0 mL sample of 0.250 M H_2SO_4 is neutralized by 20.5 mL of KOH solution. What is the molarity of the KOH solution?
- In an acid-base neutralization reaction, 23.74 mL of 0.500 M potassium hydroxide solution reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?
- If 0.900 L of 0.450 M H2SO4 is mixed with 0.800 L of 0.280 M KOH, what concentration of sulfuric acid remains after neutralization?
- If 0.950 L of 0.450 M H2SO4 is mixed with 0.900 L of 0.290 KOH, what concentration of sulfuric acid remains after neutralization?
- Determine the volume of 0.22 M KOH solution required to neutralize each sample of sulfuric acid. 1. 15 ml of 0.22 M H_2SO_4 2. 85 ml of 0.130 M H_2SO_4
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution Phases are optional. 0.550 L of 0 490 M H_2SO_4 is mixed with 0 500 L of 0.270 M KOH. What concentration of sulfu
- A volume of 80.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 13.7 mL of 1.50 M H_2SO_4 was needed? The equation is 2KOH (aq) + H_2SO_4 (aq) to K
- A volume of 80.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 16.7 mL of 1.50 M H_2SO_4 was needed? The equation is [{MathJax fullWidth='false' \r
- A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 15.2 mL of 1.50 M H_2SO_4 was needed? The equation is 2KOH (aq) + H_2SO_4 (aq) to K_
- 0.450 L of 0.490 M H_2SO_4 is mixed with 0.400 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?
- If 0.550 L of 0.440 M H2SO4 is mixed with 0.500 L of 0.260 M KOH, what concentration of sulfuric acid remains after neutralization?
- If 0.450 L of 0.400 M H2SO4 is mixed with 0.400 L of 0.290 M KOH, what concentration of sulfuric acid remains after neutralization?
- 0.650 L of 0.420 M H_2SO_4 is mixed with 0.600 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?
- If 0.650 L of 0.430 M H2SO4 is mixed with 0.500 L of 0.290 M KOH, what concentration of sulfuric acid remains after neutralization?
- 0.150 L of 0.490 M H2SO4 is mixed with 0.100 L of 0.250 M KOH. What concentration of sulfuric acid remains after neutralization?
- 0.350 L of 0.44 M H_2SO_4 is mixed with 0.3 L of 0.29 M KOH. What concentration of sulfuric acid remains after neutralization?
- 0.250 L of 0.470 M H_2SO_4 is mixed with 0.200 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?
- If 0.850 L of 0.470 M H2SO4 is mixed with 0.800 L of 0.210 M KOH, what concentration of sulfuric acid remains after neutralization?
- 0.350 L of 0.470 M H_2SO_4 is mixed with 0.300 L of 0.250 M KOH. What concentration of sulfuric acid remains after neutralization?
- A 33.00 mL sample of an H_2SO_4 solution of unknown concentration is titrated with a 0.1122 M KOH solution. A volume of 41.22 mL of KOH is required to reach the equivalence point. What is the concentration of the unknown H_2SO_4 solution?
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution. Phases are optional. 0.250 Lof 0.460 M H_2SO_4 is mixed with 0.200 L of 0.260 M KOH. What concentration of sulfuric acid...
- In an acid-base neutralization reaction 28.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H_2SO_4 solution?
- Determine the volume of 0.255 M KOH solution required to neutralize each of the following samples of sulfuric acid. The neutralization reaction is: \\ H_2SO_4(aq) + 2KOH(aq) \rightarrow K_2SO_4(aq) + 2H_2O(l) \\ Part A: 30 mL of 0.255 M H_2SO_4 Part B:
- In a titration experiment, 147.77 mL of 0.935 M KOH is reacted with H_2SO_4. The endpoint is reached when 92.77 mL of the acid is mixed with the base. What is the molar concentration of the acid?
- Titration of a 23.0 mL solution of KOH requires 13.0 mL of 0.0250 M H2SO4 solution. What is the molarity of the KOH solution?
- Titration of a 15.0 mL solution of KOH requires 17.0 mL of 0.0250 M H2SO4 solution. What is the molarity of the KOH solution?
- Titration of a 11.0 mL solution of KOH requires 11.0 mL of 0.0270M H2SO4 solution. What is the molarity of the KOH solution?
- Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution Phases are optional. 0.250 L of 0.450 M H_2SO_4 is mixed with 0.200 L of 0.280 M KOH. What concentration of sulf
- An acid solution is 0.100 M in HCl and 0.200 M in H_2SO_4. What volume of a 0.150 M KOH solution would completely neutralize all the acid in 500.0 ml of this solution?
- A volume of 40.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the solution if 19.2 mL of 1.50 M H_2SO_4 was needed? The equation is 2KOH (aq) + H_2SO_4 (aq) to K_2SO_
- What volume of 0.344 M H2SO4 solution would be required to neutralize completely 34.4 mL of 0.255 M KOH solution?
- What volume of 0.296 M H2SO4 solution would be required to neutralize completely 34.4 mL of 0.296 M KOH solution?
- A 32.00 mL sample of a H_2SO_4 solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 40.22 mL of KOH was required to reach the equivalence point. What is the concentration of the unknown H_2SO_4 solution?
- Suppose 0.750 L of 0.410 M H2SO4 is mixed with 0.700 L of 0.240 M KOH. What concentration of sulfuric acid remains after neutralization?
- Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. 0.750 L of 0.430 M H2SO4 is mixed with 0.700 L of 0.250 M KOH. What concentration of sulfuric acid remains after neutralization?
- In an acid-base neutralization reaction, 38.74 mL of 0.500 mol L-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?
- A volume of 60.0 of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 25.2 mL of 1.50M H_2SO_4 was needed? The equation is 2KOH + H_2SO_4 \to K_2SO_4 + 2H_2O
- Calculate the volume (ml) of a 0.215 M KOH solution that will completely neutralize each of the following: a) 2.50 ml of a 0.825 M H_2SO_4 solution. b) 18.5 ml of a 0.560 M HNO_3 solution.
- H2SO4(aq) + 2KOH(aq) ==>2H2O(l) + K2SO4(aq) 0.650 L of 0.440 M H2SO4 is mixed with0.600 L of 0.290 M KOH. What concentration of Sulfuric Acid remainsafter neutralization?
- A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid?
- A 27.00mL sample of an H_2SO_4 solution of unknown concentration is titrated with a 0.1422M KOH solution. A volume of 40.22mL of KOH was required to reach the equivalence point. What is the concentrat
- A 25.00-mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1328 M KOH solution. A volume of 38.33 mL of KOH was required to reach the endpoint. What is the concentration of t
- Consider the following balanced chemical reaction: H2SO4 (aq) + 2 KOH (aq) \to K2SO4 (aq) + 2 H2O (l) What volume, in L, of 0.500 M KOH solution is required to completely react with 1.32 L of 0.300 M H2SO4 solution?
- In an acid-base neutralization reaction 25 mL of 0.4 M NaOH reacts with 50.00 mL of H_2SO_4 solution. Calculate the concentration of the H_2SO_4 solution?
- Determine the volume of 0.210 M KOH solution required to neutralize each of the following samples of sulfuric acid. The neutralization reaction is: H_2SO_4(aq) + 2KOH(aq) => K_2SO_4(aq) + 2H_2O(l)
- A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 22.2 mL of 1.50 M H_2SO_4 was needed? 2 KOH(aq) + H_2SO_4(aq) to K_2SO_4(aq) + 2H_2O
- 1. Write the balanced neutralization reaction between H_2SO_4 and KOH in aqueous solution. Phases are optional. 2. 0.450 L of 0.430 M H_2SO_4 mixed with 0.400 L of 0.210 M KOH. What concentration of
- A volume of 60.0 ml of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 25.7mL of 1.50 M H_2SO_4 w
- A volume of 80.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). What was the molarity of the KOH solution if 21.7 mL of 1.50 M H_2SO_4 was
- In a titration of 26.0 ml of 0.840 M H_2SO_4, __________ ml of a 0.200 M KOH solution is required for neutralization. Express your answer to the nearest 1/10 ml. Hint: Remember H_2SO_4 is a diprotic acid.
- Suppose 0.250 L of 0.430 M H2SO4 is mixed with 0.200 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.250 L of 0.420 M H2SO4 is mixed with 0.200 L of 0.290 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.550 L of 0.460 M H2SO4 is mixed with 0.500 L of 0.220 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.550 L of 0.450 M H_2SO_4 is mixed with 0.500 L of 0.250 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.250 L of 0.440 M H2SO4 is mixed with 0.200 L of 0.220 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.750 L of 0.440 M H2SO4 is mixed with 0.700 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.250 L of 0.490 M H_2SO_4 is mixed with 0.200 L of 0.290 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.950 L of 0.450 M H2SO4 is mixed with 0.900 L of 0.240 M KOH. What concentration of sulfuric acid remains after neutralization?
- Suppose 0.750 L of 0.490 M H2SO4 is mixed with 0.700 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?
- You have 50 mL of 3.0 M H2SO4. How many mL of a 2.0 M solution of KOH is needed to exactly neutralize the acid?
- A 27.5 mL sample of a KOH solution of unknown concentration requires 14.6 mL of 0.150 M H2SO4 solution to reach the endpoint in a titration. What is the molarity of the KOH solution?
- A 30.5 mL sample of a KOH solution of unknown concentration requires 18.1 mL of a 0.100 M H2SO4 solution to reach the endpoint in a titration. What is the molarity of the KOH solution?
- A 15.5 mL sample of 0.215 M KOH solution required 21.2 mL of aqueous sulfuric acid in a titration experiment. Determine the molarity of the sulfuric acid solution.
- An acid solution is 0.120 M in HCl and 0.200 M in H_2SO_4. What volume of a 0.150 M solution of KOH must be added to 500.0 mL of the acidic solution to completely neutralize all of the acid?
- How many milliliters of a 2.61 m H2SO4 solution is needed to neutralize 71.50 mL of a 0.855 m KOH solution?
- How many milliliters of a 2.61 M H2SO4 solution are needed to neutralize 71.50 ml of a 0.855 M KOH solution?
- A 500 ml sample of solution of H_2SO_4 was titrated with 60 ml of 1.5 M KOH. What was the molarity of the H_2SO_4 sample?
- An acid solution is 0.100M in HCl and 0.210 M in H2SO4. What volume of a 0.160 M KOH solution would have to be added to 550.0 mL of the acidic solution to neutralize completely all of the acid?
- An acid solution is 0.100 M in HCl and 0.200 M in H2SO4. What volume of a 0.140 M KOH solution would have to be added to 550.0 mL of the acidic solution to completely neutralize all of the acid?
- Determine the volume of 0.215 M KOH solution required to neutralize each of the following samples of sulfuric acid. The neutralization reaction is: H_2SO_4 (aq) + 2KOH (aq) to K_2SO_4 (aq) + 2H_2O(l) 1. 15 mL of 0.215 M H_2SO_4. 2. 155 mL of 0.130 M H_2SO
- Determine the volume of 0.220 M KOH solution required to neutralize each of the following samples of sulfuric acid. The neutralization reaction is: H_2SO_4 (aq) + 2KOH (aq) to K_2SO_4 (aq) + 2H_2O (l). 1) 40 mL of 0.220 M H_2SO_4. 2) 175 mL of 0.140 M H_2
- The neutralization of 27.3 mL of H_2SO_4 solution, of unknown concentration, requires 72.2 mL of 0.12 M LiOH solution. What is the concentration of the H_2SO_4 solution (in M)?
- How many mL of a 0.0485 M H2SO4 solution is required to exactly neutralize 25.0 mL of a 0.17 M KOH solution?
- A 0.6745-gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the molarity of the KOH solution?
- A volume of 50.0 mL of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid. What was the molarity of the KOH solution if 19.2 mL of 1.50 M H_2SO_4 was needed? The e
Explore our homework questions and answers library
Browse
by subject