![Data Table 2. Solutions of Ammonium lon- Ammonia Solution [NHaCl], M Acid, base, or neutral? Experimental pH NH3], M 0.10 1.0](http://img.homeworklib.com/images/0349428e-a09e-4b8e-af88-a7741e56f62b.png?x-oss-process=image/resize,w_560)
![The concentrations of [NHaCI] and [NH3] will need to be calculated using the ICE-box method before they are entered in the ta](http://img.homeworklib.com/images/1cc6cc1d-1556-4640-8502-720031ca28fb.png?x-oss-process=image/resize,w_560)
![Table 3. Determining Ko and pKs for Ammonium ion. Solution[H30*], M [NHa], M NHACI], M Calculated Ko Calculated pKa for NHA f](http://img.homeworklib.com/images/1a2ac1da-9e08-420d-896d-27bf6dec0974.png?x-oss-process=image/resize,w_560)
The concentrations of [NHaCI] and [NH3] will need to be calculated using the ICE-box method before they are entered in the table below. Show one representative calculation. (Attach an additional sheet of paper to this lab if necessary.) 2.
Table 3. Determining Ko and pKs for Ammonium ion. Solution[H30*], M [NHa], M NHACI], M Calculated Ko Calculated pKa for NHA for NH4 589X1 -lo 4.5 Xlo 3.09x10 .22x IO -to Not req'd Not req'd
Homework Answers
![pH- pK+log[NH3l/[NH4CI] If [NHbl INH.CI] then pH-pKa Which is the case for solution Cand D. So pKa calculated is average of 9](http://img.homeworklib.com/images/b8f03163-e774-4a20-a756-15f54a09c0c4.png?x-oss-process=image/resize,w_560)
Add Answer to:
Data Table 2. Solutions of Ammonium lon- Ammonia Solution [NHaCl], M Acid, base, or neutral? Expe...
CHEM 202 Chemistry of Acids & Bases-Parts 1 and 2 College of the Canyons Data L Nt CX Table 2 . S...
Need help with calculations!!
CHEM 202 Chemistry of Acids & Bases-Parts 1 and 2 College of the Canyons Data L Nt CX Table 2 . Solutions of Ammonium lon-Ammonia Acid, base, or Experimental pH neutral? Solution [NH.cil, M INHs), M 0.10 1.0 0.050 0.05 0.50 0.10 5.81 5 .22 1. 33 10.81 0.50 Calculations 1. Determine [H,O'] ] for each solution using your experimental data above and enter the data in Table 3 below Show one representative calculation below. -.10...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-]...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
0.50 M solutions of each weak acid in the table are available. Choose an acid solution...
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in ml, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 3.94. acid base pairs to use: K på, HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 1.8*10-4 3.74 4.2x10-7 6.38 7.3x10-10 9.14 4.8x10-11 10.32 HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 ml NaOH
Critical Skills #9 (Acid-Base Equilibria) Due: 6 pm Monday March 30 upload to Gradescope Class time:...
Critical Skills #9 (Acid-Base Equilibria) Due: 6 pm Monday March 30 upload to Gradescope Class time: 9:30 pH = 11:00 (from back of page) 2:00 1. Consider the conjugate acid-base pair NH' and NH, a. Write the acid dissociation (lonization) reaction for NHA' in water. Hint: NHU (aq) + HOS Label each conjugate acid-base pair. ? 6. Write the expression for equilibrium constant for this reaction ( ?) c. Write the base dissociation (lonization) reaction for NH, in water. Hint:...
7. Fill in the table with acid/base conjugate pairs Acid/conj base Reagent Acid/Base 2 Base/conj. acid...
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...
Q(27) The pH of a 0.050 M aqueous solution of ammonium chloride falls within what range? A) 0-2 B) 2-7 C)7-9 D) 9-1...
Q(27) The pH of a 0.050 M aqueous solution of ammonium chloride falls within what range? A) 0-2 B) 2-7 C)7-9 D) 9-12 E) 12-14 Q(28) Based on the information in the table below: which acid in aqueous solution is the weakest? Name Formula Ka Acetic Acid CH3COOH 1.8X10-5 Benzoic Acid C6H5COOH 6.3 X10-5 Formic Acid HCOOH 1.7 X 104 Hydrofluoric Acid HF 7.1 X 104 A) CH3COOH B) C6H5COOH C) HCOOH D) HF Q(29) K = 2.39 for the...
Just give me the answers 14) A0.15 M aqueous solution of the weak acid HA at...
Just give me the answers
14) A0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pHi of 5.35. The value of Kg for HA is A) 14 10-10 B) 7.1 10-9 E) 33 104 918-10-5 D) 3.0 10-5 15) The Kg for HON is 49-10-10, What is the value of Kb for CN-? A) 49-10-24 B) 20 10-5 D) 4.9-104 9 4.0 10-6 E) 2.0 109 16) Caleulate the pOH of a 0.0827 M aqueous...
U Experiment 17B: Acid-Base Titration Report Data Table Trial 1 Trial 2 T Trial 3 Volume...
U Experiment 17B: Acid-Base Titration Report Data Table Trial 1 Trial 2 T Trial 3 Volume of Acetic Acid Final buret reading 42.35 27.67 Initial buret reading 30.00 38.32 5.81 32.51 30.00 44.40 3.95 40.45 Volume of NaOH 27.67 Exact Molarity of NaOH (From 17A or see label) 1252 Calculations: 1. Calculate the molarity of the acetic acid for each trial and the average molarity Trial 1: Trial 2: Trial 3: Average Molarity of Acetic Acid = 2. Use the...
I added everything thing. this is the lab question you need to solve. First assigned buffer...
I added everything thing.
this is the lab question you need to solve.
First assigned buffer pH: 2.031 Second assigned buffer pH: 9.171 Available Buffer Systems (acid/ base) pka of Conjugate Acid 2.847 4.757 malonic acid/ monosodium malonate acetic acid/ sodium acetate ammonium chloride/ ammonia triethylammonium chloride/ triethylamine 9.244 10.715 1) Buffer system details: Given pH Name and volume conjugate acid Name and volume conjugate base 2) Calculations for preparation of high capacity buffer system. Introduction In this experiment, you...
Need help with calculations!!
CHEM 202 Chemistry of Acids & Bases-Parts 1 and 2 College of the Canyons Data L Nt CX Table 2 . Solutions of Ammonium lon-Ammonia Acid, base, or Experimental pH neutral? Solution [NH.cil, M INHs), M 0.10 1.0 0.050 0.05 0.50 0.10 5.81 5 .22 1. 33 10.81 0.50 Calculations 1. Determine [H,O'] ] for each solution using your experimental data above and enter the data in Table 3 below Show one representative calculation below. -.10...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in ml, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 3.94. acid base pairs to use: K på, HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 1.8*10-4 3.74 4.2x10-7 6.38 7.3x10-10 9.14 4.8x10-11 10.32 HCO2H/NaHCO2 H2CO3 NaHCO3 H3B03 NaH2B03 NaHCO3/Na2CO3 ml NaOH
Critical Skills #9 (Acid-Base Equilibria) Due: 6 pm Monday March 30 upload to Gradescope Class time: 9:30 pH = 11:00 (from back of page) 2:00 1. Consider the conjugate acid-base pair NH' and NH, a. Write the acid dissociation (lonization) reaction for NHA' in water. Hint: NHU (aq) + HOS Label each conjugate acid-base pair. ? 6. Write the expression for equilibrium constant for this reaction ( ?) c. Write the base dissociation (lonization) reaction for NH, in water. Hint:...
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...
Q(27) The pH of a 0.050 M aqueous solution of ammonium chloride falls within what range? A) 0-2 B) 2-7 C)7-9 D) 9-12 E) 12-14 Q(28) Based on the information in the table below: which acid in aqueous solution is the weakest? Name Formula Ka Acetic Acid CH3COOH 1.8X10-5 Benzoic Acid C6H5COOH 6.3 X10-5 Formic Acid HCOOH 1.7 X 104 Hydrofluoric Acid HF 7.1 X 104 A) CH3COOH B) C6H5COOH C) HCOOH D) HF Q(29) K = 2.39 for the...
Just give me the answers
14) A0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pHi of 5.35. The value of Kg for HA is A) 14 10-10 B) 7.1 10-9 E) 33 104 918-10-5 D) 3.0 10-5 15) The Kg for HON is 49-10-10, What is the value of Kb for CN-? A) 49-10-24 B) 20 10-5 D) 4.9-104 9 4.0 10-6 E) 2.0 109 16) Caleulate the pOH of a 0.0827 M aqueous...
U Experiment 17B: Acid-Base Titration Report Data Table Trial 1 Trial 2 T Trial 3 Volume of Acetic Acid Final buret reading 42.35 27.67 Initial buret reading 30.00 38.32 5.81 32.51 30.00 44.40 3.95 40.45 Volume of NaOH 27.67 Exact Molarity of NaOH (From 17A or see label) 1252 Calculations: 1. Calculate the molarity of the acetic acid for each trial and the average molarity Trial 1: Trial 2: Trial 3: Average Molarity of Acetic Acid = 2. Use the...
I added everything thing.
this is the lab question you need to solve.
First assigned buffer pH: 2.031 Second assigned buffer pH: 9.171 Available Buffer Systems (acid/ base) pka of Conjugate Acid 2.847 4.757 malonic acid/ monosodium malonate acetic acid/ sodium acetate ammonium chloride/ ammonia triethylammonium chloride/ triethylamine 9.244 10.715 1) Buffer system details: Given pH Name and volume conjugate acid Name and volume conjugate base 2) Calculations for preparation of high capacity buffer system. Introduction In this experiment, you...
Most questions answered within 3 hours.
-
Suppose that on a temperature scale X, water boils at 203.0°X
and freezes at -105.7°X. What...
asked 6 minutes ago -
BaS crystallizes in a cubic unit cell with S2- ions on each
corner and each face....
asked 37 minutes ago -
A. 0≤P(Oi)≤10≤P(Oi)≤1 for each i
B. P(Oi)≤0P(Oi)≤0
C. P(Oi)=1+P(OCi)P(Oi)=1+P(OiC)
D. P(Oi)≥1P(Oi)≥1
If an experiment consists of...
asked 2 hours ago -
A battery has an emf of 9.20V and an internal resistance of 1.20
ohm. a)What resistance...
asked 2 hours ago -
The area of an elastic circular loop decreases at a constant
rate, dA/dt = −6.60×10−3 m2/s...
asked 3 hours ago -
The denaturation of proteins can be described by the
equilibrium
F⇌U
where F and U represent...
asked 4 hours ago -
Please answer what the maximum and minimum force is, and the
angle on the ion is...
asked 4 hours ago -
implement a program that reads a number of rows and a symbol.
The program will draw...
asked 4 hours ago -
Assume that when adults with smartphones are randomly selected,
45% use them in meetings or classes....
asked 4 hours ago -
Determine the number of formula units of
Na2SO4 and moles of oxygen contained in 8.11
moles...
asked 5 hours ago -
Explain in steps on the following code
What would be the output when executed
using System;...
asked 5 hours ago -
Given the information in the table, which of the following
statements is CORRECT?
Stock A
Stock...
asked 5 hours ago