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A 100 ml $\ce{HCl}$ solution has a pH of $3.7$. You want the solution to be of pH 4.5. You have a solution of $10\ \mathrm M$ $\ce{NaOH}$.
$\begingroup$ Do you really need to know pH or just that solution is 4.00 molar NaOH? Can you assume that the solution is "pure" NaOH? No NaCl, no KOH. I'm wondering about a sodium electrode, or conductivity. Carbonate from the air will be a problem. $\endgroup$ –
Usually, the biggest problems with preventing a sodium hydroxide solution from changing in NaOH N a O H concentration, or pH, over time are adsorption of COX2 C O X 2 from the air, and evaporation of water via permeation through the container holding the solution. If we can really say that it is inside a closed system as you've specified, then ...
$3\\cdot 10^{-2}\\ \\mathrm{mol}$ of $\\ce{NaOH}$ are added to a $1\\,\\mathrm{l}$ solution of $2\\cdot10^{-2}~\\mathrm{M}\\ \\ce{CH3COOH}$. Find the $\\mathrm{pH ...
Since 1 hydroxide ion is created from each molecule of sodium hydroxide that dissociates , hence 0.02 M NaOH will give 0.02 M of hydroxide ions. p O H = − l o g 10 (O H) − = − l o g 10 (0.02) p O H = 1.70 p H + p O H = 14 ⇒ p H = 14 − 1.70 = 12.3 p H = 12.3
You have 100 ml of NaOH @ pH 13. If you dilute by 10 times, then the new pH will be 12, so you'll need to dilute it another 10 times to reach pH 11. If you start with 100 ml, you'll need to end with 10 litres in total (100 folds). You already have your 100 ml, so you'll need to add 10000 ml −100 ml =9900 ml.
The first one is. COX2 + NaOH(aq) NaHCOX3(aq) and the second one is a two-step reaction, first with water then sodium hydroxide: COX2 + HX2O(l) HX2COX3(aq), HX2COX3(aq) + NaOH(aq) NaHCOX3(aq) + HX2O(l) So my question is which one of these answers is right? To me, I do not understand why the 2nd option takes into account water because really ...
That is, 5 moles of NaOH N a O H gives 5 moles of OHX− O H X − ions after complete dissociation. Find the equivalents of HX+ H X + from phosphoric acid (a) and the equivalents of OHX− O H X − from NaOH N a O H (b). Also calculate the total volume. Number of equivalents= NV N V. But be careful since concentration is given in molarity.
This website claims that if you add $\pu{50 mL}$ of $\pu{0.05 M}$ sodium bicarbonate, and $\pu{5 mL}$ of $\pu{0.1 M}$ sodium hydroxide (and dilute to $\pu{100 mL}$), you should create a solution with $\mathrm{pH }= 9.6$. I'm struggling a bit getting this result. My attempt: The sodium bicarbonate reaction would be:
What is pH? pH is a measure of hydrogen ion concentration to determine the alkalinity or acidity of a solution. If the pH value of a solution is less than 7 it is an acidic solution. If the pH value of a solution is greater than 7 it is a basic solution. If the pH value of a solution is equal to 7 it is a neutral solution.