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What are the possible solutions for m plus 6 is greater than or equal to 15?
[ 'm' is greater than or equal to 9 ].There are an infinite number of numbers that satisfy that solution.
How many gallons of a 90 percent antifreeze solution must be mixed with 90 gallons of 15 percent antifreeze to get a mixture that is 80 percent antifreeze?
Let M equal the gallons of the 90% mixing solution. Let F equal the gallons of the final solution. So:90 + M = F.Also, the number of gallons of pure antifreeze in the final will equal the sum of the gallons of antifreeze in the two mixing parts:Original solution: ( 90 gal )*(0.15) = 13.5 gal [0.15 represents 15%]Mixing solution: M*0.90Final solution: F*0.80So 13.5 + M*0.90 = F*0.80Now you have 2 linear equations and 2 unknowns, you can solve for M & F, using your favorite method: M = 585 and F = 675. Add 585 gallons of the 90% to get 675 gallons of 80% solution.
What is the pH of a solution withOH equals 1 10-4?
-log[1 X 10^-4 M OH(-)] = 4 14 - 4 = 10 pH ----------------
What does it mean to have the pH of a solution equal to zero?
The pH is define in the following way: pH = -log [H+] What that means is the pH is the negative of the base 10 logarithm of the concentration of hydrogen ions in the solution. So, if you have a pH = 0, that means that the concentration of H+ is equal to 1 molar, because -log(1) = 0. If you have a 1 M solution of any strong acid, the pH will be equal to zero.
Does 3m equal m m m?
No.
What is true about a solution of 1.0 M HF?
HF has a higher [OH-] than a solution of 1.0 M HCl.
What is the OH- in a solution with a pOH of 4.22?
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
What is the OH in a solution with a pOH of 4.22?
[OH-] = 1x10^-4.22 or more conventionally, [OH-] = 6.03x10^-5 M
How many grams of Na OH have been dissolved per liter of solution to make a 7.0 M Na OH solution?
ungimat
What is the OH- in an oven-cleaning solution if the pH is 12.35?
.022 M
What is the pH of a solution with a oh of 3.31 00000000 M?
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
What is the OH of a 4.0 x 10 4 M solution of CaOH2?
The OH concentration in a 4.0 x 10^4 M solution of Ca(OH)2 can be determined by dividing the concentration of Ca(OH)2 by its stoichiometric coefficient, which is 2. Thus, the OH concentration is 2.0 x 10^4 M.
If it requires 40 ml of 3.5 m naoh to neutralize 55 of hcl what is the molarity of the hcl solution?
40 ml of NaOH contains 0.04 L * 3.5 M = 0.14 mole of NaOH Since NaOH donates 1 OH you will also have 0.14 mole of OH- in solution. This can be neutralised with an equal amount of H+. HCl can donate 1 H+, so you need an equal amount of H+ to neutralise the OH-. So you need 0.14 mole of the HCl. 55 ml has 0.14 mole HCl. So the molarity is: 0.14 mole / 0.055 L = 2.54 M
Calculate the molar it’s oh a solution that contains 15.7 of CaCO3 dissolved in enough water to make 275mL of solution?
0.570 M (note the capital M, this is molarity.)
What is the molarity of OH- in an aqueous solution that is 0.34 M HNO3?
1.00 * 10^-14/ 0.34 = 2.9^-14 M or (3.2e-14 M)
What is the hydroxide ion of 4.5 x 10-7 M?
The pH of a 4.5*10-7 M OH- solution is 7.7
What is the OH- in a solution that contains 0.240 g NaOH in 0.225 L of solution?
Molarity = moles solute/Liters solution get moles NaOH 0.240 grams NaOH (1 mole NaOH/39.998 grams) = 0.0060 moles NaOH ----------------------------------as one to one OH- has this many moles also Molarity = 0.0060 moles OH-/0.225 Liters = 0.0267 M OH- ----------------------- -log(0.0267 M OH-) = 14 - 1.573 = 12.4 pH -------------
