Acid & Base
3) Sodium hydroxide (NaOH) is a base.
Sodium hydroxide, releases OH- ion, hence it is a base.
4) Hydrochloric acid (HCl) is an acid.
Hydrochloric acid releases H+ ion, hence it is an acid.
( Note: According to the Arrhenius acid- base, theory, acid is a compound that releases H+ ion, and base is a compound that releases OH- ion).
5) Dissociation reaction of sodium hydroxide and Hydrochloric acid.
i) Sodium hydroxide dissociate into sodium ion and hydroxide ion.
NaOH ---------> Na+ + OH-.
ii) Hydrochloric acid dissociate into Hydrogen ion and Chloride ion.
HCl ---------> H+ + Cl-.
Unknown solution: The solution, whose concentration is unknown is called unknown solution. ( Here solution is not mentioned, and hence cannot be answered whether it is acid or base).
8) Dissociation constant gives information about the extent of dissociation of acid or base.
The value of dissociation constant depends on the type of acid or base.
For weak acids and base, the dissociation constant is less than unity (1). ( Because weak acids or base do not dissociate completely)
For strong acid and base it is equal to unity (1). (Strong acid or base completely dissociate at all concentrations).
Both NaOH and HCl are strong base and strong acid respectively, hence there dissociation constant is equal to one.
( Rest of the questions can not be answered, as the necessary charts and information is not provided).
Acid & Base 1. Follow the acid & base experiment procedure and answer the following questions 2- Watch t...
Dissociation Ethanoic Acid Hydrochloric Acid Nitric Acid Phosphoric Acid Universal solution Universal chart (enter label here) pH Meter Dissociation 1- Follow the dissociation experiment procedure and answer the following questions. 2- Identify which of these acids which are provided in the experiment are strong acids or weak acids and why? (look at the reaction details bax) By using the pH universal chart and solution 3- Write down the pH value for each acid. 4- Does 1 M of strong acid...
Titration: Acids and Bases 2. How can you determine which acid is diprotic? 3. using the answers to questions one and two, which acid is diprotic? 4. Which base has more hydroxide ions per molecule? Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
Use this description to answer the questions: Solution 1 is 0.1M weak acid HF and the pH is found to be 2.8. Write the acid dissocation reaction for HF. Solution 2 consists of the same 0.1 M weak acid HF but in 1.0M sodium nitrate. Write T if the statement is true, F if it is false. The pH of solution 1 and solution 2 will be the same within statistical error. The pH of solution 2 will be lower...
1 a) Write the aqueous acid dissociation reactions for an acid and base dissociation reaction for a base according to the Bronsted-Lowry definition b) Determine conjugate bases of acids and acids of bases c) Write the equilibrium expression for an acid or a base aqueous dissociation d) Evaluate strength of an acid or base based on its Ka or Kb or pKa or pKb. e) Apply Kw at 25oC and at different temperatures. f) Solve for the pH of strong...
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
7. Fill in the table with acid/base conjugate pairs Acid/conj base Reagent Acid/Base 2 Base/conj. acid -но o9uenn H SO HOHSO 4 Hq ibnit t boau noisup orl ai t W CI +H O HCI+OH HOT b n tad HCI +NH CI +NH 3 NH +HO NH +OH 2 MO1701 List 3 strong acids and explain why these acids are considered strong acids. a. b. 8. с. eniwollol odi lo doso to Ho pdod bluow ai List 3 weak acids...
Questions: 1. Write balanced equations for each of the four different acid-base reactions in this experiment. Include phases (s, 1, g, aq) for reactants and products. Naoteit HChagj- NaOH agl+ NH2 (09) t HUiagy NHz 491 HadtNaa (a4) Hao t NaCats HCaHso (44) NH4 ca) + C211202a) t 2. How does the enthalpy of neutralization change when you switch from a strong acid to a weak acid with the same base? From a strong base to a weak base with...
100 Experiment 12 Determination of Solution pH 2. Provide equations for each of the following. (Use compounds from question 1. if you want a) Dissociation of a strong base in water b) Dissociation of a strong acid in water c) lonization of a weak base in water d) lonization of a weak acid in water e) Autoionization of water _ M 3. A 5.0 M solution of HCl in water has a proton concentration of M. 4. A 0.01 M...
± pH of a Strong Acid and a Strong Base pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10−14 where 1.00×10−14 is the value at approximately 297 K. Based on this relation, the pH and pOHare also related to each other...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...