We have 2.89 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 8.73 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution?
We have 2.89 L of an aqueous NaBr solution. We add an excess of AgNO3. We...
Question 2 : We have 2.80 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 9.53 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution?
To a 88.8 mL aqueous solution of NaOH, we add an excess of Mn(NO3)2 and produce 0.090 g of Mn(OH)2(s). What was the original pH of the NaOH solution?
13. What is the molarity of a 2.66 L aqueous solution containing 56.9 g of NaBr? 14. If 3.08 g of Ca(OH)2 is dissolved in enough water to make 0.875 L of solution, what is the molarity of the Ca(OH)2? 15. What mass of HCl is present in 825 mL of a 1.25 M solution? 16. What mass of isopropyl alcohol (C3H8O) is dissolved in 2.050 L of a 4.45 M aqueous C3H8O solution?
Question A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion. Ag+...
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion....
Determining the amount of sulfate ion (SO2) dissolved in seawater in the unit of molarity QUESTION Sulfate concentration in the seawater is about 28 mm (0.028 M). Take the reverse approach to the calculation procedure in the previous Question #1 (so called a backward calculation) and find a rough estimate for the volume of the seawater sample you may need to take from the beach like the one below. A 20.0 mL sample solution contains unknown amount of bromide ion...
Calculate the concentration of an aqueous KCl solution if 246 mL of the solution gives 28.5 g of AgCl when treated with excess AgNO3. The equation for the reaction is KCl(aq) + AgNO3(aq) ----> AgCl(s) + KNO3(aq)
16 Cts with aqueous copper(II) chloride accord- 101. Zinc metal reacts with aqueous copper(1) ing to this equation: Zn (s) + CuCl2 (aq) → ZnCl2 (aq) + Cu (s) In this reaction, what mass of copper metal can be pro- duced from the reaction of 500 mL of 1.20-M aq. cu 2 with excess zinc? 10 103. The concentration of bromide ion may be determined by gravimetric analysis, using this reaction: Ag+ (aq) + Br (aq) → AgBr (s) A...
Which of the following can donate a proton, H+, to water? ОКСІ OHI CH4 O AgNO3 Question 13 Determine which of the following has the highest oxidation state for vanadium. 0 V2O5 O VO2 OVO o V203 Which of the following can accept a proton, H+, in aqueous solution to form a polyatomic ion? O HCI О КОН O KBr Ο ΝΗ3 Question 15 What is the net ionic equation for the reaction between aqueous sodium hydroxide and aqueous hydrobromic...
1) Write the solubility-product expression for the following mercury salts: Hg2Cl2 and HgCl2. 2) Exactly 0.133 mg of AgBr will dissolve in 1.00 L of water. What is the value of Ksp for AgBr? 3) By experiment, it is found that 1.2 x 10-3 mol of lead (II) iodide, PbI2, dissolves in 1.0 L of water at 25°C. What is the Ksp at this temperature? 4) What is the molar solubility of silver chloride in 1.0 L of solution that...