1) Show the calculation for determining the mass of NaOH pellets required to prepare 250mL of 0.10M NaOH. 2) What substance is the proton donor and which is the proton acceptor in NaOH and KHP? 3) What is an equivalence point in a titration?
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
1. How many grams of CI2 can be prepared from the reaction of 15.0 g of MnO2 and 30.0 g of HCl according to the following equation? 2. How many mL is 0.005 L? 3. Give the number of protons (p), electrons (e), and neutrons (n) in one atom of chlorine - which has the symbol Cl. 4. A newborn baby weighs eight and one ha
I know that: 2HCL +Fe(s)= FeCl2 + 2H under normal conditions. I want to know if the concentrations or conditions can be altered to produce: 3HCl + Fe(s)=FeCl3 + 3H using NO other reactants (catalysts may be used).
From what I have gathered, it appears that the reaction between Iron and certain acids can produce either Fe2+ OR Fe3+ ions. For example, I believe that HCl and Fe(s) will produce hydrogen and either FeCl2(aq) AND/OR FeCl3(aq). Similiarly, the reaction between Fe(s) and H2SO4 will produce hydrogen and Iron (II) sulfate(aq) A
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 →
Draw the new structure of lidocaine with the two molecules produced and its new functional groups after hydrolysis.
10.0 mg of AgOH(s) is added to 350.0 mL of water with an initial pH of 11.00. The solubility equilibrium constant for the dissolution of AgOH (s) is Ksp = 1.5 x 10^-8. Determine the concentration of [Ag +] and the final pH at equilibrium.
Boric acid, B(OH)3, is an acid that acts differently from normal Bronsted-Lowry acids. It reacts with water to form B(OH)4- and H30+. a) Draw Lewis structures and indicate the shapes for B(OH)3 and B(OH)4- b) What is the species that donates a proton to water? c) Can B(OH)3 be described as a Lewis acid?
A. What is the pH of a solution in water with a concentration of H3O+ ions of 3.5x10^-8M. Is this solution acidic or basic? B. A solution in water has a pH of 5.25. What is the molarity of H3O+ ions in this solution?
Human blood plasma is approximately 0.70% NaCl by weight. What is the ionic strength of blood plasma? I need a detailed explanation please- not just numbers! I am using this as a study guide for my final. Thnaks!!
How many metric tons of 5%-S coal would be needed to yield the H2SO4 required to produce a 5.0 cm rainfall of pH 2.00 over an area of 100 square kilometers? Hint: calculate the volume of rain, mol H+, mass of S, mass of coal. If you could work out the problem for me, that would be great! It makes it easier to understand.
A weak base with Kb=4.240*10^-7 is added to water to make a 2.00*10^-1 M solution. what is the pH? Since Kb is small, can assume that the dissociation is small relative to initial concentration of weak base.
For which type of titration will the ph be basic at the equivalence point? Show work. Thanks
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
Balanced Reaction: Ti(OH)4 + 2H2SO4 ---> Ti(SO4)2 + 4 H20 - Name each reactant,and product. What type of reaction is this? What is the limiting reagent? - How many grams of water can be produced from this reaction? Show the calcuation of the molar masses of the necessary substances before showing the calculation for theor
What is the concentration of 25.0 mL of HCl if it is completely neutralized by 47.4 mL of 0.250 M NaOH?
Complete each reaction. In(OH)3 (s) + HF (aq) ----> BaCO3 (s) + HNO3 (aq) ----> NH3 (aq) + H3PO4 (aq) ----> Nb(OH)2 (s) + HBr (aq) ---->
In the lab you add excess hydrochloric acid (HCl) to 2.65 g of Na2CO3. Complete and balance the reaction, and identify the state of each substance.
Show the complete, balanced reaction when 2.35 grams of Ti(OH)4 reacts with excess sulfuric acid.
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.
Please see the attached file for full problem description. show work and all steps for problem, thanks for your time
What is the pH of a 2.5 mol HCL / liter aqueous solution?
Please see the attached file for full problem description. Show work and all steps, thanks for your help.
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
Question: You are asked to go into the lab and prepare an ethanoic acid - sodium ethanoate buffer solution with a pH of 4.00 ± 0.02. What molar ratio of [CH3COOH] / [ CH3COONa] should be used?
Question: Which one of the following combinations cannot function as a buffer solution? HCN and KCN NH3 and (NH4)2SO4 HONO2 and NaNO3 HF and NaF HONO and NaNO2
7 general chemistry questions. Example: At 20 degrees Celcius, the vapor pressure of toluene is 22 mm Hg and that of benzene is 75 mm Hg. An ideal solution, equimolar in toluene and benzene, is prepared. At 20 degrees Celcius, what is the mole fraction of benzene in the vapour in equlibrium with this solution? (a) 0.23 (b)