**11 use pH and Ka to find initial concentration YouTube**

The initial pH will be significantly less than 7 in this case for any significant initial concentration of acid, and as NaOH is added, the pH will increase since OH - is a …... This equation shows the final step of a process to find the pH of a solution composed of water and a weak acid. C is the initial concentration of the weak acid before it dissociates.

**Calculate initial concentration when given pH? Yahoo Answers**

Create an ICE chart that expresses the initial concentration, the change in concentration, and the equilibrium concentration for each species in the reaction. From the chart you can determine the changes in the concentrations of each species and the equilibrium concentrations. From the example, we start with the folowing information.... This is the concentration of hydronium ions, so to find the pH, all we have to do is take the negative log of that. So, the pH is equal to the negative log of the concentration of hydronium ions. So we can just plug that into here: 5.3 x 10-6, and we can solve; and let's take the - log(5.3 x 10-6) And so we get: 5.28, if we round up, here. So let me get a little more room... So we're rounding

**homework Finding the initial concentration - Chemistry**

pH is - log[H+] where [H+] is the hydrogen ion concentration in moles per liter. (Technically it is the activity, which is slightly lower in concentrated solutions, but for most common purposes you can use the concentration.) how to find my netflix password on ps3 To find a concentration of hydronium ions in solution from a pH, we use the formula: \[[H_3O^+]= 10^{-pH}\] This can be flipped to calculate pH from hydronium concentration:

**How do you find the initial acid concentration of an**

24/09/2011 · Best Answer: use this question to help you :) calculate the pH of a 0.176M solution of a weak acid with a pKa of 3.121" ANSWER pKa = 3.121 Ka = 10^ -3.121 = 0.000757 For the equilibrium HA <> H+ + A- initial concentration 0.176 at equilibrium 0.176-x . . x . . . .x 0.000757 = (x )( x) / 0.176-x x = 0.0115 M how to find standard error on ti 84 Note the conversion of significant figures between concentration and pH - the number of significant figures in the concentration becomes the number of decimal places in the pH value (and vice versa), since pH is a logarithmic scale. So in the examples above, 2 significant figures of accuracy in the concentration data results in 2 decimal places of accuracy in the resultant pH values.

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### How to calculate molar concentration when a pH is given

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## How To Find Ph Of Initial Concentration

pH is - log[H+] where [H+] is the hydrogen ion concentration in moles per liter. (Technically it is the activity, which is slightly lower in concentrated solutions, but for most common purposes you can use the concentration.)

- 26/02/2010 · Calculating initial concentration of a weak acid given pH and Ka? Calculating Ka & initial concentration of an unknown acid from pH? Calculate concentrations given Ka and pH? More questions. Calculate concentration given pH and Ka? Calculate pH of weak acid given concentration? Answer Questions . 9.54 g of a compound has decomposed to give 8.98 g of O. The rest is H. If the …
- This is the concentration of hydronium ions, so to find the pH, all we have to do is take the negative log of that. So, the pH is equal to the negative log of the concentration of hydronium ions. So we can just plug that into here: 5.3 x 10-6, and we can solve; and let's take the - log(5.3 x 10-6) And so we get: 5.28, if we round up, here. So let me get a little more room... So we're rounding
- So if you enter the values for initial concentration and KA’s for various acids into columns of a spreadsheet Excel can, in a new column, calculate the H + from: =(-K1+SQRT(K1^2+4* I1*K1))/2
- The value of K b1 is small enough to assume that C is small compared with the initial concentration of the carbonate ion. If this is true, the concentration of the CO 3 2- ion at equilibrium will be roughly equal to the initial concentration of Na 2 CO 3 .