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If you dissolve 2.2 g of the same Colgate toothpaste in 100 mL water, a) What is the molarity of NaF in this solution? b) What is the molarity of fluoride ion in this solution? c) What is the concentration of NaF in this solution, in ppm? d) What is the concentration of fluoride ion in this solution, in ppm?
If 32.0 g CaC2 are consumed in this reaction, how many moles of H2O are needed?
At what temperature is the reduction of tungsten(VI) oxide by hydrogen to give metallic tungsten and steam spontaneous? The standard heat of formation of WO3(s) is -843 kJ/mol, and its standard molar entropy is 76 J(K mol).
Can someone please explain this to me. My answer was Na+
Problem- The following are the half lives of four active isotopes. Which one of the following is the most dangerous to handle
calculate the equilibrium partial pressures of CO2 and CO.
The reaction 2COF2 (g) CO2 (g) + CF4 (g) has an equilibrium constant of Kc = 2.20x10^6 at 292 K. Determine the value of the equilibrium constant for the reaction 2CO2 (g) + 2CF 4 (g) 4COF2 (g)
The thermite reaction is given by- Fe2O3(s) +Al(s) ------> Fe(l) + Al2O3(s). Explain how many grams of molten iron will be produced if 2.29 moles of iron (III) oxide is consumed
What mass of NaCl must be dissolved in 65.0 grams of water to lower the freezing point by 7.50 °C? The freezing point depression constant, Kfp, for water is -1.86 °C/m. Assume the van't Hoff factor for NaCl is 1.87.
a experiment would also work using another reactive metal such as zinc.If you had used the same number of grams of Zn as you did Al in this experiment,would you have obtained more or less hydrogen. Illustrate with an equation and calculation
Gibbs Free Energy and Equilibrium The reaction SO2(g)+2H2S(g)?3S(s)+2H2O(g) is the basis of a suggested method for removal of SO2 from power-plant stack gases
If the vapor pressure of ethyl ether and ethyl alcohol at 20°C are 375 torr and 20.0 torr, respectively, the vapor pressure of the solution at 20°C
An 80-proof brandy is 40.0% (v/v) ethyl alcohol. The "proof" is twice the percent concentration of alcohol in the beverage
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