Sodium bicarbonate was added to an unlimited amount of sulfuric acid undergoing a reaction to produce sodium sulfate plus carbonic acid (which turned in to water vapor and carbon dioxide upon heating). Please provide a balanced equation for this reaction.
1. Write a balanced equation for the reaction of calcium phosphide with water to produce phosphine and calcium hydroxide, in a atmosphere of carbon dioxide at 0C and a pressure of 4.8mm Hg. At STP carbon dioxide has a density of 1.96g/litre, and phosphine has a density of 1.53g/litre. Liquid water is used in the reaction. 2.
The following acid-base reaction is performed in a coffee cup calorimeter: H+(aq) + OH-(aq) --> H2O(l) The temperature of 110 g of water rises from 25.0°C to 26.2°C when 0.10 mol of H+ is reacted with 0.10 mol of OH-. * Calculate qwater * Calculate ΔH for the reaction * Calculate ΔH if 1.00 mol
Observations: 1) A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2. 2) B does not react with any of the 1mol/L solutions above or the dilute sulfuric acid. 3) C reacts spontaneously with dilute sulfuric acid and with 1mol/L solutions of all the other metallic
Could you please explain what happens when hydrogen ions are added to a mixture of barium chromate (S) and chromate ions (AQ). Would there be a precipitate and, if not, why?
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 + 2.5E10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHa? What is pKa of the acid component? I don't understand this problem at all! I know that a diprotic substance has something i
I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer. The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I ca
Question 31 What is the molarity of a solution in which 26.0 grams of BaCl2 (molar mass = 208.2 g/mol) are dissolved in enough water to make 450.0 mL of solution? 0.278 M 0.617 M 1.00 M 3.41 M Question 32 Which element has the following electron configuration? 1s22s22p63s2 Na Mg
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 = 2.5E-6. In order to make up a buffer solution of pH 5.8, which combination would you choose, NaHA/H2A or Na2A/NaHA? I know the solution is Na2A/NaHA, but I am not sure why. What is the pKa of the acid component?
A diprotic acid, H2A, has the following ionization constants: Ka1=1.1E-3 and Ka1=2.5E-6. In order to make up a buffer solution of pH 5.80, which combination would you choose: NaHA/H2A or NA2A/NaHA? I know this is NA2A/NaHA, but don't know why. What is the pKa of the component?
How much NaOH is needed to prepare 576 mL of solution with a pH 10? Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)? Is the concentration of a solution the same as the concentration of [OH-] or [H+]?
Please provide the exact steps that are involved in solving each of these problems and how to arrive at the answers step-by-step so I can grasp the concept clearly. 1. The gaseous hydrocarbon acetylene, C2H2, is used in welders torches because of the large amount of heat released when acetylene burns with oxygen, producing ca
A weak acid has a pKa of 3.654. If the solution pH is 3.741, what percentage of the acid is undissociated? A weak acid has a pKa of 5.857. Calculate the pH of a solution in which the ratio of the concentrations of acid anion to undissociated anion ([A-]/[HA]) equals 7.555.
Please help, I'm really stuck on the following:- A weak acid has a PKa of 7.713. Calculate the pH of a solution in which the ratio of the concentrations of undissociated acid to acid anion ([HA]/[A-]) equals 8.441 also Calculate the PKa of a weak acid given the information that a 0.652 M solution has a pH of 2.882
1) When iron is oxidized in the presence of nitric acid, three products are formed: iron(III) nitrate, nitrogen dioxide and water. Write and balance the equation for this reaction. Then calculate how many grams of water are formed if 500 grams of iron are reacted with 500 grams of nitric acid. 2) When iron is oxidized in th
The only possible ions in an aqueous solution are ion, barium, carbonate, chloride and nitrate. The following are observed: i) the original solution contains only dissolved species. ii) adding silver ion to the solution produces no precipitates. iii) adding sulfate ion to the original solution produces a white precipitate
14. In a normal bottle of Coca Cola before it is opened, the following equilibrium exists: H2C03 <=> H+ +HCO3-; Ka = 4.2 x 1 O-7 Once the bottle is opened, this equilibrium no longer exists. Explain what happens, and write a new equilibrium expression showing what happens. I'll give you a hint; there is more than one equil
Please see the attachment for complete information. 15. Into a 5.0 liter flask was placed 35.7 g of PCI5 . The flask and contents were heated to 250 0 C, and then held at temperature until the following equilibrium was established: PcI5 (g)< > Pc13 (g) + Cl2 (g) It was then shown by analysis that 875 g of Cl2 was pesent
During titration the following data were collected. A 50mL portion of an HCl solution was titrated with 0.50 M NaOH. It required 200mL of the base to neutralize the sample. How many grams of acid are in 500 mL of this acid solution? The attached solution describes all steps of the required procedure to find out the unkonwn a
Reactions of metals with acids and metal ions. 1. What are the equations for these metals when mixed with 6 M HCl. Ca, Cu, Mg, Fe, Sn, and Zn. (I tried Ca + HCl and got 3 Ca + 6HCl --> 3CaCl2 + 3H2) 2. We have Ca(NO3)2, Cu(NO3)2, FeSO4, Fe(NO3)3, Mg(NO3)2, SnCl4, and Zn(NO3)2. What is the complete equation and net ion
Brass is an alloy of copper and zinc.When ground into a fine powder,then added to hydrochloric acid solution,a single replacement reaction occurs with one of the metals.A soluble salt and hydrogen gas are produced. A)The balnce equation for the reaction that occurs? B)If a 60.0 g sample of the alloy contained enough of the m
What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1 liter of solution buffered at Ph of 3.55?
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 and pH is 4.20. a. Calculate the concentration of C6H5NH3+ in this buffer solution. b. Calculate the Ph after 4.0 grams of NaOH(s) is added to 1.0 L of this solution. Neglect any volume change.
I need a simple way of telling if an acid is strong or weak (by looking at the formula). I need the same explanation for bases.
Question: If 500 mg/L lactic acid is added to pure water and you add NaOH until the pH = 3.1, what are the final amounts of each species in the acid equilibrium? What is the titratable acidity? The formula for lactic acid is C3H603, with a dissociation constant, pKa = 3.86. The formula for tartaric acid is C4H606. We us
1) How many moles of chloride ions are in 250.0mL of a 0.450M calcium chloride solution? 2) Identify the spectator ions for the reaction: CuBrsub2 (aq) + Lisub2CrOsub4(aq) -> CuCrOsub4(s) + 2LiBr(aq)
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
1. Calculate the Ksp of a saturated solution if it contains 0.0001 M Pb2+. 2. CH2ClCooH(aq) --(Forward/Reverse reaction)--H+ (aq) + CH2ClCOO- (aq) Calculate the value of Ka(acid) if a 0.1 M solution of CH2ClCOOH has a pH of 2. (a.) given pH, what is the [H+]? (b.) given [H+], what is [CH2ClCOO-]? (c.) Wha
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?