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1. What would be the pH of a solution of 1.56gm of hydrochloric acid in 2250 ml of solution?
2. How many mols of nitric acid would be in 1375 ml of the acid solution at a pH of 3.75?
3. What would be the [H+] and [OH-] of a solution at pH=10.50?
What mass of zinc in grams is required to produce 3.2L of H2 (g) from the following reaction at 78 degrees celcius and 790mmHg? Please explain
What techniques might you employ to induce crystallization if no crystals have formed after you cool the solution to room temperature.
what is the final temperature of 100 g of water, initially at 20 Celsius , to which 1000 calories (cal) are added
A stock solution is prepared by adding 25 mL of 2.2 M AlCl3 to enough water to make 75 mL. What is the Cl- concentration of 25 mL of the stock solution.
A reaction in which and react to form products is zero order in , one-half order in , and second order in .By what factor does the reaction rate change if is doubled
Write down the reactions that occurred in each test tube if no reaction occurred then put NR on the product side Test tube.
which ions in water make it 'hard'? is it possible to test for only one of these ions quantitatively in the presence of the other.
The product formed is 2-hexanol, is this an example of 1,4 addition, or proceeds via a carbanion, or is an example of electrophillic addition, or results in sp2 hybridized carbon being transformed into a sp hybridized carbon?
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and .0280 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate
when 56.0 g calcium and 34.7 g nitrogen gas undergo a reaction that has a 88.0 yield what mass of calcium nitride
an evacuated empty 276 ml glass bulb weighs 129.6375 g. filled with an unknown gas the bulb weighs 130.0318 g.
A sample of nitrogen gas in a 4.5-L container at a temperature of 27 C exerts a pressure of 4.1 atm. Calculate the number of moles of gas in the sample
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