4. a) Write the equation for the reaction of sulfuric acid with potassium hydroxide. b) If Ms. Chemist has a solution of potassium hydroxide that is 0.68 M, what is the volume (in mL) of the base needed to react completely with 55.0 mL of 2.45 M sulfuric acid? c) How many grams of acid were needed to make up the acidic sol
21. One gram of NaCl and one gram of sand are added to 100mL of water. What is the solvent? NaCl Sand Water The Na and Cl ions 22. The gradual mixture of one gas with another by kinetic energy is termed diffusion. True False 23. Which of the following compounds is an acid? H2O N2
Using Ostwald process, what mass of nitric acid could be produced from 75.0 g of N2 and 50.0 g of H2? I have all the molar masses, the limiting factor, and the ratio of the limiting factor to the product. How do I put this information into an equation to come up with a reasonable answer?
Commercial steric acid (C17H35COOH) contains palmatic acid (C15H31COOH) as an impurity. If a 1.115 gram sample of commerical steric acid is dissolved inm 43.95 grams of benzene, the freezing point is found to be 5.072 degrees celcius. If the freezing point of pure benzene is 5.533 degrees celcius what is the percent by mass of
Write a chemical equation for the following reactions: i) zinc sulphate + barium nitrate ii) gold (III) sulphate + barium chloride iii) zinc + mercourous nitrate iv) tin + antimony (V) chloride v) calcium + water vi) ferrous bromide + phosphoric acid vii) calcium carbonate + hydrobromic acid →
In the lab you add excess hydrochloric acid to 2.65g of Na2CO3. The balanced reaction is 2HCL (aq) + Na2CO3 (aq) ---> CO2 (g) + H20 (l) + 2NaCl (aq) 1) Identify the type of reaction 2) How many grams of gas molecules can be formed from this much Na2CO3? Show the calculation of the molar masses of all necessary substances
Question: 5.0 mL of 12 mol NH3 / Litre solution is added to 500.0 mL of 0.050 mol AgNO3 / Litre solution. Assume the combining volumes are additive, What molar concentration of silver ion will exist in solution after equilibrium is established? Ag+ + 2 NH3 = Ag(NH3)2+ ( Kf for Ag(NH3)2+ is 1.5 x 107 ) P
1. Write net ionic equations to correspond with each of the following molecular equations. (a.) HCl(aq) + NaOH(aq) NaOH(aq) + H2O(l) (b.) Na2CO3(aq) + CoCl2(aq) 2 NaCl(aq) + CoCO2(s) (c.) NH3OH(aq) + CH3COOH(aq) CH3COONH4(aq) + H2O(l) 2. Define the following terms: (a.) conjugate acid-base pairs (b.) self-ionization
What mass of potassium hypochlorite must be added to 450.0 mL of water to give a solution with pH = 10.20? Please see the attached file for full problem description.
Over what range of pH is a HOCl - NaOCl buffer most effective? pH 2.0 - pH 4.0 pH 7.5 - pH 9.5 pH 6.5 - pH 8.5 pH 6.5 - pH 9.5 pH 1.0 - pH 14.0
Objective: To study the effect of reactant concentration on the rate of the reaction between sodium thiosulfate and hydrochloric acid and to determine the order of each reactant and the rate law for the reaction. 2 HCI(aq) + NaS2O3 (aq) --> S(s) + SO2 (aq) + H2O(l) + 2NaCL(aq) Calculations: (a) Calculate the initial an
A compound of iron and oxygen is found to have a mass of 6.13 grams. If the mass of iron is determined to be 4.29 grams, what is the empirical formula of the compound? Please give step by step answer in simplest way to do not making it complicated. Show all steps and solution please.... (See attachment for rest of question
List the following in order of increasing pH of their 0.1 M aqueous solutions (lowest to highest pH) NaBr NH4Br NaClO2 NaBrO2
Question: What is the pH of 0.097 M of triethylammonium chloride (CH3CH2)3 NHCL? I know that in order to solve this i need to find the Kb, which is equal to Kw/Ka, I know that Kw = 1E-14, but I do not know which Ka to use? Once i know the Kb, i will be able to solve this problem and find the pH, i just need help finding the a
Following netralization reaction H2SO4 + KOH ->
Compare the vapor pressures of methanol,ethanol,acetic acid, water, and benzene. Which compund appears to have the strongest intermolecular forces at 100C If one compound has a higher equilibrium vapr pressure than another at a particular temperature, will it necessarily have a higher equilibrium vapor pressure at all tempe
127. Calculate the temperature (K) of the earth if there were no greenhouse effect. Assume the solar irradiance is 1500 W/m2 and the total planetary albedo is 25 percent. (The Stefan Boltzmann constant is 0.567e-07 W/m2/K4). ****I've tried to answer this twice, but both times I was incorrect and the program gave the following h
1. 0.54 g of ammononium chlordie is dissolc=ved in 250 mL of solution. Calculate the molarity. 2. What volumne of solution would be required to deliver 6.84 g og 0.200 M aluminum sulfate solution? 3. Calculate the molarity of a solution if 126 mL of 6.25 M NaOH was diluted to a total volume of 250mL. 4. Calculate the pH
103897 okay if expalin math Only for above listed OTA-ONLY. All others called in. Please EXPLAIN the math. 100 mL of a 0.1 M NaOH solution is being titrated with 0.2 M HCl solution. a) What is the pH of the solution after 25 mL of the HCl solution has been added? b) What is the solution after an additional 20 mL of HCl solut
Please show all work and remember this is a first year course. Chem is my weakest subject. Please send responsse in Word. Also, if you are not willing to show me the proper way to do these by showing the calculations and will only supply me with some notes tht I could read out of any textbook myself, please do not take th
Everything is already answered I just need to know if I am on the right track, please help I am really struggling with chemistry and I absolutely need to know how to do these problems correctly, so if I am wrong can you please tell me were my error is. ----------- Which of the following salts would give you the lowest co
1. Conjugate Acid-Base Pairs. Identify the conjugate acid-base pairs in each of the following reactions. Label each species as an acid or a base. a. NH4+(aq) + CN-(aq) --> NH3(aq) + HCN(aq) b. CH3COOH(aq) + F-(aq) --> CH3COO-(aq) + HF(aq) c. HPO42-(aq) + H2O(l) --> H2PO4-(aq) + OH-(aq) d. NH3(aq) + SO4 2-(aq) --> N
I) At 25ºC, 0.212g of barium hydroxide is dissolved completely in sufficient water to make 0.25 liter of final solution. What is the hydroxide ion concentration in mol litre-1? Given answer in scientific notation to an appropriate number of significant figures. ii) What assumption must you make in order to carry out the cal
A solution is prepared by mixing 46.8 mL of 0.16 M Pb(NO3)2 with 75.3 mL of 1.4 M KCl. Calculate the concentrations of Pb2+ and Cl- at equilibrium. Ksp for PbCl2(s) is 1.6 10-5.
At 25 degrees C, 0.212 g of barium hydroxide is dissolved completely in sufficient water to make 0.25 liter of final solution. What is the hydrogen ion concentration (in mol/liter) in this solution? What is the pH of this solution (to the nearest integer)
Arrange the following five reduction half-cell reactions in order listing the largest positive reduction potential first and give the best oxidizing and reducing agents. Observations: i) A reacts spontaneously with 1 mol/L BNO3, 1 mol/L D(NO3) and dilute sulfuric acid. A does not react 1 mol/L C (NO3) ii) B does not re
When microorganisms reproduce they release waste products that may change the pH and prevent further reproduction. Therefore culture mediums for growing microorganisms are usually buffered. The median for the culture of lactobacilli includes a buffer prepared by dissolving 25 grams K2HPO4 and 25 grams KH2PO4 in water and dilut
a) Write a balanced equation for the reaction of aluminium selenide with water to Hydrogen selenide and solid aluminium hydroxide (including physical states) showing the sequence of partially balanced equations needed, including a brief description of the strategy used. b) The density of hydrogen selenide at STP is 3.61 g lit
How do you calculate the percent disagreement using a calculator for 1.01x10^19 (Avogrado's number of oleic acid molecules /mol (theoretical result being Avogrado's number)? Please be specific because I am not quite sure how to do this on the calculator.
A 0.10 M Mn 2+ solution is saturated with H2S. At what pH will MnS begin to precipitate? [H2S] sat'd=0.10M