What is a reactive compound and state two examples?
I have a 2 part question concerning the use of H2SO4 to adjust the pH of a solution: 1. How many grams per liter of H2SO4 is required to adjust the pH of a solution from 3.8 to 2.8 assuming the sulfuric acid fully ionizes? 2. If in reality however, the actual sulfuric acid ionization/dissociation is a 2 step process and no
Assume we have a 1000L tank of water and very dilute weak acids. To this tank we add and dissolve 260 grams AL2(SO4)3 (solid granules) --- the resultant pH is 4. The intention is to form AL(OH)3 solids/particles in this reaction. Question 1: How much Al(OH)3 will be formed in this reaction at pH=4.0 Question 2: If the pH w
The only problems that need to be done are numbers (3) and (4) on the second scanned document and the question below . Numbers (1), (2), (5) are finished problems that do not need to be done so problems (3) and (4) should be done using the same format (do Calculations and preparation)as those. Also please answer this ques
Please help with the following problems. a.) Giving the reason for your answer, which would you expect to have the higher value of pH, a 1.0M solution of the strong acid, HCl or a 1.0M solution of the weak acid, acetic acid, CH3COOH? b.) Why is it that we can say that ozone in the stratosphere is beneficial to
1. A solution is prepared by dissolving 10.8g ammonium sulfate in enough water to make 100.0mL of stock solution. A 10.00mL sample of this stock solution is added to 50.00mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. 2. One of the most commonly used white pigments in paint
Acid content of vinegar Flask 1 Flask 2 Inital volume of NaOH in burette 0 17.5 Final volume of NaOH in burette 17.5 35.3 Volume of NaOH used for titration
Zn(OH)2 is amphoteric. In which of the following solutions would the solubility of Zn(OH)2 be lowest and why?
Zn(OH)2 is amphoteric. In which of the following solutions would the solubility of Zn(OH)2 be lowest and why? a) pure water b) 1 M ZnCl2 C) 1 M NH3 d) 1 M NaOH e) 1 M HCI
PH OF A BASIC SOLUTION. PH is defined as the negative logarithm of Hydrogen ion concentration. Strength of a base is expressed as the concentration of OH- ions. Therefore PH of a basic solution can be calculated using the relation Kw=[H+][OH-]=1x10-14 at 25degree celcius PH=-log[H+] Problem: Calculate the PH of a s
1) Pennies made after 1982 contain 97% zinc by mass. A student wants to prove this by filing the copper outside the penny until he sees zinc and then putting the penny in a 1.00 M HCl solution. The zinc will be oxidized and the H+ (from the HCl) will be reduced: Zn + 2H+ ----- Zn2+ + H2 If the entire pen
1) Given the following two equations, determine the number of grams of manganese dioxide required to prepare enough chlorine gas to produce 25.0 g of potassium hypochlorite. MnO2 + 4HCl ----- MnCl2 + Cl2 + 2H2O Cl2 + 2KOH ------ KCl + KClO + H2O 2) A titration is done us
Please show how to solve the following questions: 2Al (s) + 2KOH (aq) + 4 H2SO4 (aq) + 22 H2O (l) --> 2KAl (SO4)2*12H2O (s) + 3H2 (g) 12.0 g of Al, 420 mL 2.0M KOH, 216 mL H2SO4 placed in 300 mL ice bath (water in excess) 1) What is the limiting reagent? 2) How much aluminum is necessary to produce 18g of alum? 3)
Write a balanced chemical equation, include states of matter: 5 drops 0.1M MgSO4 to 5 drops of 0.1M BaCl2 Write a balanced chemical equation, include states of matter: 2 mL saturated Na2CO3 solution to 5 drops of 6M HCl
1) Write a balanced chemical equation, include states of matter: 5 drops of 0.1 M NaCl solution to 5 drops 0.1 M AgNO3 solution 2) Write a balanced chemical equation: About 10 drops of 6M NH3 to the AgCl formed in (1) (which dissolves the AgCl) 3) Write a balanced chemical equation: About 10 drops of 3M HNO3 to the p
Solid aluminum hydroxide Al(OH)3 (s) reacts with aqueous sulfuric acid H2SO4 (aq) to produce aluminum sulfate Al2(SO4)3 (aq) and water. We combine 30.0g of Al(OH)3 (s) and 75.0 ml of 2.00 M H2SO4 (aq), and the reaction goes to completion. Subsequent analysis reveals that 12.3 g of Al2(SO4)3 was formed. What is the percent yield
Problem 1: Citric acid is concentrated in citrus fruits and plays a central metabolic role in nearly every animal and plant cell. How many moles of citric acid are in 1.90 qts of lemon juice *d=1.09 g/ml* that is 6.62% citric acid by mass? Problem 2: Nitrogen *N*, phosphorus *P*and potassium *K* are the main nutrients
1. How many significant figures does the sum of the following contain? 8.520 + 2.7? 2. How many moles of oxygen atoms are there in 10 moles of KCIO3? 3. The oxidation number of N in NaNo3 is? 4. What element is oxidized in the following chemical reaction? 3Cu + 8HNO3 ----> Cu(NO3) + 2NO + 4H2O 5. At what temp. will
Define an acid and a base in terms of the hydrogen ion.
Acetic acid (CH3COOH) is a weak acid with the following ionization reaction: CH3COOH + H2O Û H3O+ + CH3COO- Ka = 1.8 x 10-5 What is the pH of a solution that is 0.5M in acetic acid and 2.5M in sodium acetate, CH3COONa?
What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.1 M sulfuric acid? a. 9.4 mL solution b. 9.4 L solution c. 16 mL solution d. 16 L solution
(See attached file for full problem description) --- 1. Fe²+ and Sb³- 2. Mg²+ and As³- 3. Al³+ and O²- 4. Co³+ and I- 5. Sr² + and P³- 6. Ca²+ and C4+ 7. Fe³+ and As³- 8. Na + and S² ˉ Write the name or formula for these compounds: 1. tin (II) acetate 2. bromous acid 3. copper(II) permanganate
1. Butyric acid is responsible for the odor in rancid butter. It has one weakly acidic proton. A solution of .25 M butyric acid has a pH of 2.71. Determine the Ka of the acid. 2. Ka for HCN is 4.0 x 10^10. Calculate Kb for CN. 3. For the equilibrium, CH3OH (g) <-- --> CO (g) + 2 H2, Kc is 6.9 x 10-2. At equilibriu
Q#1 (Common ion problem) What is the solubility,in mg/mL of BaF2 in a)Pure Water b)in a solution containing 5.0mg/mL of KF Ksp of BaF2=1.0*10^-6 Q#2 Effect of pH on solubility a)Calculate the solubility of a saturated solution og Mg(OH)2 on pure water.(My answer is 1.65096*10^-4M b)Calculate the solubility of the sa
50.00 mL of a 1.00 M solution of the diprotic acid H2A (Ka1= 1.0 * 10^-6 and Ka2 = 1.0 * 10^-10) is being titrated with 2.00 M NaOH . How many mL of 2.00 M NaOH must be added to reach a pH of 10?
Using Hess' Law of additive equations, rearrange and/or multiply the following reactions in order to find the enthalpy for the radical reaction between hydrochloric acid and isopropyl alcohol (CH3CHOHCH3) to form water and isopropyl chloride. The dots you see indicate a radical, which is much different than an ion or an element
(See attached file for full problem description) --- 1. Tooth enamel consists of hydroxyapatite, Ca5(PO4)3OH (Ksp = 6.8x10-37). Fluoride ion added to drinking water reacts with Ca5(PO4)3OH to form the more tooth decay-resistant fluorapatite, Ca5(PO4)3F (Ksp =1.0x10-60). Fluoridated water has dramatically decreased cavities
I would like to see the details of the calculations. For my lab experiment I have the following data: Titration 1: 25.00mL of unknown concentration HCl 2 drops of phenolpthalein to show end-point 1.0M NaOH What is the molarity of the HCl? What is the Ka of the HCl? What is the equivalence point? What is the half-equival
3. Why does pH affect the solubility of CaF2 but not CaCl2? 4. Write the correct expression for Ksp for Al(OH) 3. (See attached file for full formatting)
1. Calculate the pH after 25.0 mL of .20 M HF (Ka=6.8 10-4) are titrated with 15.0 mL of .10 M NaOH? 2. Calculate the pH after 25.0 mL of 2.0 M HF is titrated with 50.0 mL of 1.0 M NaOH?
Note: You may assume that the densities of all solutions are 1.00 g/mL unless stated otherwise 1. A 10.00-mL sample of a solution containing the weak acid, formic acid, was placed in a 25-mL volumetric flask and diluted to the mark with water. A 10.00-mL sample of the diluted formic acid solution was then titrated with 0.13