0.950 L of 0.420 M H2SO4 is mixed with 0.900 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?

1) what properties of the atmosphere make it particularly suspectible to small amounts of contaminats?

2) Write the apprioprate chemical equations that governs the concentration of NO in the atmosphere if equilibrum were maintained between NO,NH3,H2O and O2. Important: place O2 on the right hand side of the reaction. the equilibrum constant for the reaction is 10^-84.03

3) Calculate the partial pressure of NH3 as if the reaction is controlled by chemical equilibrum.

What is the redox of:

ClO^- (aq) + IO₃^- (aq) → ClO₃^- (aq) + I₂ (s) [A]

What is the pH electrode response time, if the response time is considered to be 90% of the total signal change? Discuss

A 44.7 mL sample of a 0.280 M solution of NaCN is titrated by 0.220 M HCl. Kb for CN- is 2.0×10-5. Calculate the pH of the solution:

(a) prior to the start of the titration

(b) after the addition of 28.4 mL of 0.220 M HCl

(c) at the equivalence point

(d) after the addition of 83.6 mL of 0.220 M HCl.

PLEASE SHOW ALL WORK

From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2X ⟶ Y + Z

Time (s) [5.0] [10.0] [15.0] [20.0] [25.0] [ 30.0] [ 35.0] [40.0]

[X] (M) [0.0990] [0.0497] [0.0332] [ 0.0249] [0.0200] [0.0166] [ 0.0143] [ 0.0125]

Consider the reaction: 2N2O(g) ---> 2N2(g) + O2(g)

A. Express the rate of reaction in terms of the change in concentration of each of the reactants and products.

B. In the first 15.0s of the reaction, 0.015mol of O2 is produced in a reaction vessel with a volume of 0.500L. What is the average rate of the reaction during this time interval?

C. Predict the rate of change in the concentration of N2O during this time interval. In other words, what is ∆[N2O]/∆t?

How many grams of sodium acetate should be added into a two-liters buffer solution already containing 1 mole of acetic acid so as to prepare the solution with a final pH value of 4.0? The pKa of acetic acid is 4.75.
Furthermore, if you are required to adjust the aforementioned solution to a new pH value of 5.0, how many grams of NaOH should be added into the solution?

Be sure to answer all parts. Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are ingredients of baking powder that react with each other to produce CO2, which causes dough or batter to rise: Ca(H2PO4)2(s) + NaHCO3(s) → CO2(g) + H2O(g) + CaHPO4(s) + Na2HPO4(s)[unbalanced] If the baking powder contains 31.0% NaHCO3 and 35.0% Ca(H2PO4)2 by mass: (a) How many moles of CO2 are produced from 9.66 g of baking powder? mol CO2 (b) If 1 mol of CO2 occupies 37.0 L at 350°F (a typical baking temperature), what volume of CO2 is produced from 9.66 g of baking powder?

I was wondering if I was doing a conversion right. I am supposed to take aqueous HNO3 with a density of 1.42 g/mL and a mass percent of solution of 70% and convert that into molarity. Would the correct conversion be to take 70 g of HNO3 over 100 g of H2O multiplied by 1 mol HNO3 over 63.01 g HNO3 (the molar mass) and then multiply that by 1 g H2O over 0.001 L of H2O to get the moles per liter or would I use the given density (1.42 g/mL) from the problem? Also, would the molality be 11.1 mol HNO3/kg H2O and would the mole fraction be 1/6 mol HNO3/mol H2O

The fizz produced when an Alka-Seltzer® tablet is dissolved in water is due to the reaction between sodium bicarbonate (NaHCO3) and citric acid (H3C6H5O7): 3NaHCO3(aq)+H3C6H5O7(aq)→3CO2(g)+3H2O(l)+Na3C6H5O7(aq) In a certain experiment 1.25 g of sodium bicarbonate and 1.25 g of citric acid are allowed to react.

Part C How many grams of the excess reactant remain after the limiting reactant is completely consumed?

Express your answer using two significant figures.

A hypothetical element consists of two isotopes of masses 70.95 amu and 72.95 amu with abundances of 30.9% and 69.1%, respectively. What is the average atomic mass of this element?

Menthol is a crystalline substance with a peppermint taste and odor. When 0.461 g of menthol is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 2.46 °C. The freezing point and Kf constant for cyclohexane can be found here. Calculate the molar mass of menthol.

Kf= 20.8   (C⁰ /M)

Freezing point= 6.59 (C⁰ )

A buffer is constructed by dissolving 2.05 grams of sodium benzoate (144.11 g/mol) and 2.47 grams of benzoic acid (122.12 g/mol Ka = 6.50 x 10^-5) in 150.0 mL of distilled water.  The solution is titrated with 0.500 M NaOH. Calculate the pH of the solution:

a) at the equivalence point  

b) 20.00 mL NaOH before the equivalence point  

c) 20.00 mL NaOH after the equivalence point