HCI was titrated with 0.1 M KOH. The acid solution had a volume of 30.0 mL and molarity of 0.05 M. Find the pH at the following volumes of base added Volume of Titrant pH (must be in 2 (mL) decimal places) Only one answer will be considered so round off only your final answer

HCI was titrated with 0.1 M KOH. The acid solution had a volume of 30.0 mL and molarity of 0.05 M. Find the pH at the following volumes of base added Volume of Titrant pH (must be in 2 (mL) decimal places) Only one answer will be considered so round off only your final answer

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 80QAP

See similar textbooks

Related questions

Q: Activity 1. Lewis Structures Instructions: Draw a Lewis structure for: (a) H2S, (b) OF2, (c)…

A: Lewis structure :- Formulas or structures used for representation of bonds and lone pairs in any…

Q: kindi give the IUPAC name

Q: CaCl(aq) + 2 AgNO3(aq) Ca(NO3)hl ) + 2 AgCI( ) Select all the species that would be shown in the…

A: Balanced chemical reaction CaCl2 (aq) + 2 AgNO3 (aq) → Ca(NO3)2 (aq) + 2AgCl (s) In solution,…

Q: 5. What are the IUPAC names of these compounds CH,CH, (а) СН,СHCH,СНCH,CH CH, CI (b) CH,CH,CHCHCHO…

A: For IUPAC naming following steps are required- First of all identify the longest carbon chain…

Q: Part C: Ideal Gas Law (Calculation) Directions: Solve the following problems. Show your solution. 1.…

A: Ideal gas equation is given by, PV = nRT P - Pressure V - Volume n - number of moles R -…

Q: OH viii. ii. Br +En 6. X. 7. ix.

A: Alcohol is converted into alkyl-bromide with HBr Dehydrohalogentation with bulkier base like…

Q: For a galvanic cell constructed using a graphite cathode and a graphite anode : 5Sn²+ aq) + 2MnO4…

A: Galvanic cells: The cells in which chemical energy is converted into electrical energy is said…

Q: CH30 OCH3 ŅCH3CH3 22

Q: Propose stepwise mechanism of following reaction.

Q: give full and condensed electron configurations, partial orbital diagrams showing valence electrons…

A: To write: full and condensed electron configuration. Partial orbital diagram showing valence…

Q: The threshold frequency vo describes the smallest light frequency capable of ejecting electrons from…

Q: Calculate the molarity of a magnesium hydroxide solution if 23.6 mL of solution is neutralized by…

A: Molarity : Molarity is one of the concentration unit. It is defined as at a particular temperature…

Q: A student proposed two ball-and-stick models (see the image) for the XeF4 molecule, however, only…

A: The bond pair of electrons and lone pair of electrons decide the geometry of the molecules.

Q: Give a full discerption of luminescence and fluorescence. Then in short sentence what is the…

A: We have to tell about the luminescence and fluorscence. Then, we also have to tell the difference…

Q: What is E° (celI) for the cell Mn | Mn2*(aq) || Ag*(aq) | Ag? E° (V) Standard Reduction Potentials…

Q: In an acid-base reaction, a strong acid will form a weak base. True False

A: Acid is substance which release hydrogen ions and base is substance which release hydroxyl ions when…

Q: A base that does not gain H + easily is called: a. weak base b. concentrated base c. strong…

A: Define, Brønsted-Lowry theory,

Q: A certain shade of blue has a frequency of 7.12 × 1014 Hz. What is the energy of exactly one photon…

A: Frequency = 7.12 × 1014 Hz. Planck's constant = 6.626 × 10-34 J.s Energy of one photon = ?

Q: Calculate the equilibrium concentrations of the following in a 0.100 M oxalic acid, (COOH)2…

A: Given, Molarity of H2C2O4 = 0.100 M First acid dissociation constant of H2C2O4 = Ka1 = 5.9 x 10-2…

Q: Two different compounds have the formulation CoBr(SO4)·5NH3. Compound A is dark violet, and compound…

A: Here we have to predict the types isomerism shown by the following compounds having molecular…

Q: Make a systematic process for the synthesis of the benzene derivative from benzene. Present all the…

Q: 21. Which of the following involves a change of state in matter? * a. Adding food color to water b.…

A: 21.) Change is state involves conversion of state from Solid - liquid - gas . 22.) Naphthalene…

Q: Calculate the percent dissociation of propionic acid (C,H,CO,H)in a 0.20M aqueous solution of the…

Q: Propose a structure for this dianion and suggest why it forms so rea

Q: Which of the following (assuming the same concentration in water) would make a solution with the…

A: Strong acid: Strong acids completely dissociate into their ions in water. Let HA is strong acid then…

Q: c) Complete the following reaction scheme for structures E, F, G, H and I. F Br2 / H2O Cl i. BH3,…

A: Reagent KOH gives elemination reaction with alkyl halide because KOH is strong base

Q: Calculate the pH at the following points in a titration of 40.0 mL of 0.100 M barbituric acid (Ka =…

Q: a) Classify the following compounds as aromatic, antiaromatic, or nonaromatic. Give reasons for each…

Q: What is the activity coefficient for each ion at the given ionic strength at 25 °C? Activity…

Q: For a 25.0 % m/v MgCl2 solution. 1. What is the molarity ? The GFW for magnesium chloride is 95.21…

A: Here we are required to find the Molarity and osmolarity of 25%m/v of MgCl2

Q: Which of the following is NOT a property of bases? a. forms a precipitate with most metal ions…

A: Which of the following is NOT a property of bases?

Q: 6. A gas mixture contains 5 x 10°mole CO and has a total of 1 mole. What is the CO concentration in…

Q: 29, An electron in the hydrogen atom make a transition from the ground state to an excited level by…

Q: Suppose 2.94g of H2 and 2.34g of He are trapped in 2.65L container at standard temperature.…

Q: 2. Find the value for the equilibrium constant, K, at 25 °C (298 K) for the following reaction. The…

A: Given that - Temperature =298K Free energy (∆G°)= -13.6 kJ…

Q: Given the following reactions: Anode: NO3- + 2H+ + e- --> NO2 + H2O Cathode: 2H+ + 2e- - --> H2…

Q: Given the reaction: 2 HCl + Mg(OH)2 → MgCl2 + 2 H2O A student found that it required 22.0 mL of a…

Q: 10. Some of the reported chemical concentrations of water at the pH 7.3 are the following: [Na"] =…

A: We will calculate the total hardness of water in mg/L CaCO3 .

Q: EXERCISE Find (p?) for the ground state of a particle in a three-dimensional box. (Answer: h² /41².)

Q: Chan the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

Q: Which of the following ions are always present in an acidic solution? a. hydronium ions b.…

Q: What is the hybridization of the central atom in the sulfur tetrafluoride (SF) molecule?

A: Hybridization of the central atom in the SF4

Q: QUESTION 5: Sixty grams of FeCl, react with 50.0g of H,S and produced HCI. 2FEC1,(s) + 3H,S(g)…

Q: A 0.3005g sample containing Na2CO3 and NaOH requires 11.5 mL of 0.1055 M HCl to reach the…

Q: detailed mechanism of action of bisphenol A

A: Other chemicals including bisphenol S (BPS) and bisphenol F (BPF) have been evaluated as an…

Q: Use the References to access important values if needed for this questie A sample of oxygen gas…

A: Given-> V1 = 7.81 L T1 = 43.0°C = 43.0 + 273 = 316 K P1 = 1.16 atm V2 = 6.25 L P2 = 1.57 atm T2…

Q: Use the information below to answer questions 34 and 35. Elements Subatomic Na Ca Ar Particles…

A: Number of prorton gives the atomic number Sum of number of proton and neutron gives atomic mass.

Q: 10. Calculate the pH at the equivalence point for the following titration: 0.20 M HC1 versus 0.20 M…

A: Weak base (WB) and its salt with strong acid will acts as like basic buffer Basic buffer pH can…

Q: The equilbrium constant, Ke, for the following reaction is 0.215 at 673 K: NHẠI(s) NH3(g) + HI(g)…

A: Partial pressure of solid components is equal to one

Q: a photon. The wavelength of the photon is 95 E the electron can reach?

A: Given, Wavelength (L) = 95.0 nm =95×10-7 cm Initial energy level (n1) = 1 fina energy level (n2) =…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

PLEASE ANSWER 1ST AND 2ND ON THE TABLE ONLY. THANK YOU

HCI was titrated with 0.1 M KOH. The
acid solution had a volume of 30.0 mL
and molarity of 0.05 M. Find the pH at the
following volumes of base added
Volume of Titrant pH (must be in 2
(mL)
decimal places)
Only one answer
will be considered
so round off only
your final answer
15
15.5
20

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 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

A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?
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?
A 50.0-mL sample of NaHSO3 is titrated with 22.94 mL of 0.238 M KOH. (a) Write a balanced net ionic equation for the reaction. (b) What is [HSO3-] before the titration? (c) Find [HSO3-], [SO32-], [OH-], [K+], and [Na+] at the equivalence point. (d) What is the pH at the equivalence point?
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
A solution consisting of 25.00 g NH4Cl in 178 mL of water is titrated with 0.114 M KOH. (a) How many milliliters of KOH are required to reach the equivalence point? (b) Calculate [Cl-], [K+], [NH3], and [OH-] at the equivalence point. (Assume that volumes are additive.) (c) What is the pH at the equivalence point?
Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
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.