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)
1) Calculate the pH when equal volumes of 0.100 M of H2PO3- and 0.02 M HCl are mixed. 2) Calculate the percentage dissociation of acetic acid at pH = 3.69.
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
In a labratory. A solution of Ammonium chloride was given, for us to find the concentration by techniques of back titration. NaOH was added to the diluted ammonium chloride and heated. Then Titrated with HCL adding few drops of bromocresol green indicator. Colour turned yellow. What does this mean? I have done the calculation.
Will an acid-base reaction with an equilibrium lying to the right place if Na(+) A(-)is added to HB? (HB has a pka = 10):if it's needed to answer the question.
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
Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. A sodium hydroxide solution was standardized by titrating 28.71 mL of 0.1822 M standard hydrochloric acid. The initial buret reading of the sodium hydroxide was 2.70 mL and the final reading was 30.33 mL. What was the molarity
A buffer is prepared by mixing 0.027 L of 0.029 M sodium bicarbonate and 0.021 L of 0.022 M NaOH. What is the pH?
Question: A buffer is prepared by mixing 0.056 L of 0.032 M sodium bicarbonate and 0.0200 L of 0.010 M NaOH. What is the pH?
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 ->