How many kilocalories must be absorbed by the system for 6.50 liters of 1.75 M KOH...
7. How many liters of 0.775 M solution can be prepared from 55.0 g of ammonium iodide? Calculate the volume, in milliliters, of 0.468 M sodium sulfate solution to provide 2.50 g of sodium sulfate. 8. 9. How many milliliters of water should be added to 30.0 mL of a 4.00M solution to obtain a solution with a concentration of 0.200 M. 10. How many grams of AgPO4 can be produced from the reaction of 2.50 L of 0.200M AgNO,...
8. How many liters of H, gas (at STP) is produced from 470 mL of 0.36 M HCl and excess Zn? The reaction is: Zn(s) + 2 HCl(aq) - ZnCl(aq) + H (8) Hint: moles Zn(M-mole/L) then moles H2 (Bal Equ) then LH (Imole - 22.4L)
How many liters of 0.547 M koh will be needed to raise the ph of 0.223L of 4.77 M absorbic acid to a ph of 11.11?
1. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 2. How many liters of 1.75 M HCl will be required to reach the equivalence point with 1.25 L of 2.5 M KOH 3. Titration reveals that 11.6 mL of 3.0 M sulfuric acid is required to neutralize the sodium hydroxide in 25.00 mL of NaOH solution. What is the molarity of the NaOH solution? 4. Titration...
(a) In the electrolysis of aqueous Na2O2, how many liters of
H2(g) (at STP) are generated by a current of 94.0 A for a period of
87.5 min? The unbalanced chemical reaction representing this
electrolysis is shown below.
(b) How many moles of NaOH(aq) are formed in the solution in
this process?
(a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a current of 94.0 A for a period of 87.5 min?...
How many liters of 0.669 M KOH will be needed to raise the pH of 0.339 L of 4.01 M carbonic acid (H2CO3) to a pH of 9.727? Ka=5.6×10–11
How many liters of 0.810 M HNO3 are needed to react with 2.9 g of Hg2Cl2? molar mass = 472.08 g/mol Hg2Cl2 + 5HNO3 ⟶2Hg(NO3)2(aq) + HNO2(aq) + 2HCl(aq) + H2O(l)
Zinc reacts with hydrochloric acid according to the reaction equation shown. Zn(s)+2HCl(aq)⟶ZnCl2(aq)+H2(g) How many milliliters of 6.50 M HCl(aq) are required to react with 4.45 g of an ore containing 39.0 % Zn(s) by mass?
How many liters of H2 gas would be produced when a 100.0 mL solution of 165.8 mM HCl is reacted with excess zinc as described by the reaction below? Assume a temperature of 31.2C and a pressure of 1.199 atm. Express your answer in liters using at least three significant figures. Zn (s) + 2 HCl (aq) ⟶ ZnCl2 (aq) + H2 (g)
2. How many liters of hydrogen (Hz) gas can be produced from the reaction of 0.750 g of zinc (Zn) metal with excess HCl at STP. Zn (s) + 2 HCl(aq) + H2(g) + ZnCl2 (aq)