Questions: 1. Write balanced equations for each of the four different acid-base reactions in this experiment....
Please write the net ionic equations for the following acid-base reactions. HCl reacting with NaOH NaHSO4 reacting with NaOH HCl reacting with NH3 NaHSO4 reacting with NH3 (potentially helpful information: HSO4(^-) is a weak acid. HCl and NaOH are strong electrolytes)
1. Write balanced equations for the two reactions that will be carried out in this experiment HCL) + NaOH(aq) -----> HCION + NH3(04) -----> Also write a balanced equation for this reaction: NaOH + NH4Clao --> speriment #7 Pre-Lab Questions Write balanced equations for the two reactions that will be carried out in this experiment HCl + NaOH) ---> Na Clcag)+ H2O (you don't Show using Hess's Law how the enthalpy of reaction for HCl + NaOH need specific numbers,...
Please answer parts II & III. Page 63 for reference is also attached. Part IlI: Write out two chemical equations for the reactions which were performed in the hydrolysis of acetamide. See page 63. Be sure to include the names of all reactants and pro ducts. How do these reactions support your data (odors and pH)? Part IV: Write out the two chemical equations for the reactions which were performed in the hydrolys and products. How do these reactions support...
NAME INSTRUCTOR DATE SECTION GROUP POST-LABORATORY QUESTIONS THERMOCHEMISTRY: ACID-BASE NEUTRALIZATION 1. Use Hess's Law and the class enthalpy values for the reactions of NaOH-HC and NH, HCl to calculate the enthalpy of neutralization of ammonium chloride and hydrochloric acid. You may need to reverse or multiply the chemical equations from Table 7.2 and 7.3 to get them to add up correctly: Experiment Chemical reaction (Refer to the reactions that you wrote in prelab question 3). Class enthalpy value (kJ/mol 7.2...
1) Recognizing acid-base reactions. Write equations for the following acid-base reactions and predict (either by trends or by checking pKa values) which side the equilibrium prefers: a. CH3OH + NaNH2 b. HCl + H2O c. KOCH3 + HCN d. HCOOH + NaOH
Acid & Base 1. Follow the acid & base experiment procedure and answer the following questions 2- Watch the atom viewer for sodium hydroxide and hydrochloric acid then write what you observe. 3. Is sodium hydroxide acid or base and why? 4- Is hydrochloric acid or base and why? 5. Write the dissociation reaction for sodium hydroxide and for hydrochloric acid. 6- What is Unknown Solution 2 in the experiment represents acid or base and why? 7- Write the name...
PRE-LAB ACID-BASE TITRATIONS Use your textbook or lecture notes to help you write balanced equations for the reactions you will be performing in this laboratory experiment: A. HCl with NaOH B. CH3COOH with NaOH 2. For the reactions above, what are the mole to mole ratios in the balanced equations? HCI :NaOH : CH3COOH: NaOH : 2. What is the molarity of a solution of HCl if 0.2500 L of 0.2200 M NaOH is required to neutralize .1000 L of...
4. You will conduct the two solvation reactions and three neutralization reactions in this experiment. In the space provided below, write the balanced net ionic reaction equations from the descriptions. Use the table of thermodynamic data in your text (AHf(NaOH(s)= -425.61 kJ-mol) to calculate the molar enthalpy of the reactions. These will be the accepted values you will compare to the experimental values you calculate using data collected during the experiment. Part I: Solid sodium hydroxide is combined with water...
1. Write balanced equations for the chemical reactions between each acid [hydrochloric (HCI), acetic acid (CH3COOH), and citric acid (H3C6H507)] and NaOH. Note that citric acid is triprotic, which will change the balance of the chemical equation. 2. Calculate how much 0.2 M NaOH wil be needed to titrate each of the acids. Each acid is 0.1 M.
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...