Answered: It was found that 36.06 mL of HNO3…

It was found that 36.06 mL of HNO3 solution are needed to react completely with 25.0 mL of 0.19 M LIOH solution that has a pH of 13.29. What is the molarity of the HNO3 solution? [HNO3] = M

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 90QAP: A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His...

See similar textbooks

Related questions

Q: The pKa of NH4Cl is 9.2. Its conjugate base is NH3. One has two stock solutions. One is 0.1 M NH4Cl…

A: Solution contains NH4Cl and NH3.NH3 is weak base and NH4Cl is corresponding salt of strong acid. so…

Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: Answer:- Henderson-Hasselbach equation :- This equation is used for the determination of pH or pOH…

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

Q: You have 100mL of 0.1M HCI in a beaker and you begin to add NaOH to the beaker. Consider the…

Q: 4. Aqua regia (1:3 mixture of nitric acid and hydrochloric acid) is commonly used to remove noble…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00357 M HIO4 pH = (b)…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the other…

Q: 7a Calculate the pH of a solution if its [H;O*] is 5.5 x 106 7b Calculate the [OH] of a solution…

Q: Acetominophen, HC8H8NO2 (MM=151.17 g/mol), is the active ingredient in Tylenol, a common pain…

A: The question involves concept of equilibrium. we have been given pH of the solution. We have to…

Q: 150.0 mL of 2.50 M NaOH is added to a 200.0 mL solution of 1.80 M HF. Assume that the volumes are…

Q: If 0.050 moles of gaseous HCl is bubbled in 1.0 liter of a solution that is 0.15 M in NH3 and 0.10 M…

Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: GIVEN: Mass of NaC2H3O2=8.5 gVolume of NaC2H3O2=100 ml To solve: ml of 1.0M HCl needed to prepare a…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.000726 M HClO4 pH =…

Q: If 0.050 moles of gaseous HCl is bubbled in 1.0 liter of a solution that is 0.15 M in NH3 and 0.10 M…

A: When an acid is added to a weak base buffer solution, the concentration of weak base decreases where…

Q: What is the approximate pH of a 0.02 M solution of a strong monoprotic acid? Of a 0.02 M solution of…

A: Molarity of monoprotic acid=0.02MMolarity of Strong base(KOH)=0.02M

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00251 M HIO4 pH = (b)…

Q: alculate the pH of each of the following buffered solutions: 0.25 M acetic acid CH3COOH (Ka = 1.8 x…

A: Given,Concentration of Acetic Acid = [CH3COOH] = 0.25 MConcentration Sodium acetate = [CH3COONa] =…

Q: Which one of the following values of [OH-] and pH is correct? A. 1.50 g of LiOH in 250. mL of…

A: 1.50 g of LiOH in 250. mL of solution has [OH-] = 0.251 M and pH = 0.601 Molar mass of LiOH =…

Q: when 100 ml of a .01 M Mg(OH)2 solution is mixed with 100 mL of a .01 M HCl solution, what is the pH…

A: Since both acids and base are strong hence they will react to form water as shown below Mg(OH)2 + 2…

Q: 3) a) How many milliliters of 0.150 M NaOH solution are required to titrate 40.0 mL of a 0.100 M…

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

Q: What is the pH of a solution that is prepared by adding 30.23 mL of 1.77 M NaOH to 0.646 L of 0.476…

A: THIS WILL FORM AN ACIDIC BUFFER AS THE AMOUNT OF WEAK ACID(HN02)WILL REMAIN IN EXCESS AFTER REACTION…

Q: Calculate pH of the following solutions: 0.25 M HNO3 in 0.065 M CH COOH (K.=1.75x10).

A: Solution: We know the common ion aslo affect on oH of the solution. Here first we need to draw an…

Q: a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: How many milliliters of 0.0334 M KOH are needed to completely neutralize the HCI in 430 mL of a…

A: The neutralization reaction between NaOH and HCl is KOH (aq) + HCl (aq) -------> KCl (aq) +…

Q: How many milliliters of 0.0416 M KOH are needed to completely neutralize the HCI in 260 mL of a…

A: The neutralization reaction between NaOH and HCl is KOH (aq) + HCl (aq) -------> KCl (aq) +…

Q: What is the pH when 60.0 mL of 0.100 M NaOH has been added to 50.0 mL of 0.200 M HBrO? Ka or HBrO =…

Q: 4. Twenty milliliters of 0.50 N HOAC is diluted with water to 100 mL, and the resulting solution is…

Q: It was found that 27.53 mL of HNO3 solution are needed to react completely with 20.0 mL of 0.00026 M…

A: Vomume of HNO3 (V1) = 27.53 mL Vomume of LiOH (V2) = 20.00 mL Molarity of LION (M2) = 0.00026 M…

Q: a) Enough of a monoprotic acid is dissolved in water to produce a 1.291.29 M solution. The pH of the…

A: 1) we have to calculate the value of Ka for the weak acid

Q: what is the pH of the solution if 16.0 mL of 0.100 M NaOH is added to 20.0 mL of 0.150 M HCl? Is the…

Q: In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products…

A: Given ,

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

It was found that 36.06 mL of HNO3 solution are needed to react completely with 25.0 mL of 0.19 M LIOH solution that has a pH
of 13.29. What is the molarity of the HNO3 solution?
[HNO3] =
M

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: to determine

VIEW

Step 2: determine the molarity of HNO3

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
The weak base, CIO (hypochlorite ion), is used in the form of NaCIO as a disinfectant in swimming pools and water treatment plants. What are the concentrations of HCIO and OH and the pH of a 0.015 M solution of NaCIO?
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
For which of the following solutions must we consider the ionization of water when calculating the pH or pOH? (a) 3108M HNO3. (b) 0.10 g HCl in 1.0 L of solution. (c) 0.00080 g NaOH in 0.50 L of solution. (d) 1107M Ca(OH)2. (e) 0.0245 M KNO3
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
At 25 C, a 0.10% aqueous solution of adipic acid, C5H9O2COOH, has a pH of 3.2. A saturated solution of the acid, which contains 1.44 g acid per 100. mL of solution, has a pH = 2.7. Calculate the percent dissociation of adipic acid in each solution.