Ph Definition and 512 Threads

Homework Statement NaOH is an example of a strong base. if 0.45g of NaOH is mixed with 500ml of water what is the [OH] [H3O+] pH Homework Equations The Attempt at a Solution so, i calculating moles thru molar mass and divided by 0.5 to get mol/l. put that as the...

Homework Statement Prior to introducing livestock, a fishkeeper may establish colonies of nitrosifying and nitrifying bacteria by repeatedly inoculating an aquarium with a solution of ammonia (to simulate the presence of fish). At the end of the process there is a high concentration of...

Homework Statement Calculate the volume of 0.116 M HCl(aq) required to neutralize the following solutions. all the hydroxide ions in 25.0 mL of 0.215 M KOH(aq) 1. What is the molarity of Cl - ions at the stoichiometric point? Homework Equations HCl + KOH --> KCl + H2O The...

Homework Statement What volume of solution is needed to dissolve 1.0 mol of a strong base such as KOH to make a solution whose pH is 12.5? Homework Equations KOH_{(s)} \rightarrow K^{+}_{(aq)} + OH^{-}_{(aq)} pH = -log[H_{3}O^{+}] The Attempt at a Solution I'm not going to...

Homework Statement When carbon dioxide "dissolves" in water, essentially all of it reacts to form carbonic acid, H2CO3: CO2(s) + H2O(l) <--> H2CO3(aq). The carbonic acid can then dissociate into H+ and bicarbonate ions, H2CO3(aq) <--> H+(aq) + HCO3-(aq). Consider a body of otherwise pure...

Homework Statement A 100.0mL buffer solution is 0.175M in HClO and 0.150M in NaClO. Find the pH of the solution.Homework Equations Ka=10^-pH ([H30+][A-])/([HA]) -log([H30+]) = pH The Attempt at a Solution [HClO] [H3O+] [ClO-] I .175 0 .150 C...

If water were is heated to aproximately 90C will the water at this temperature have a different PH level to water at room temperature? Thanks,

I am conducting a wine analysis experiment for my undergraduate biochemistry course and am a bit stuck on the influence of pH on yeast function. Why does a high H(+) concentration kill the yeast or inhibit its growth/metabolisation of the glucose? I am guessing that the hydrogen ions somehow...

I was making some wine recently for my undergraduate biochemistry course and i have to explain why the pH of the wine decreased during fermentation. I am genuinely at a loss; what is responsible for this decrease in pH?

Homework Statement Calculate the ph of a buffer made by mixing 50.0 mL of 0.10M of acetic acid with 50.0 mL of 0.10M sodium acetate. Use the Henderson-Hasselbalch equation. Homework Equations pH = pKa + log ([base]/[acid]) The Attempt at a Solution I know how to do this problem...

Homework Statement Sulfuric acid (H2SO4) were collected from the waste acid container and the volume is 350 l. Homework Equations a) Calculate the acid pH of the solution when the hydrogen ion concentration is 2.0 ∙ 10-4 mol / l. The Attempt at a Solution i think it's simple no ...

Homework Statement A swimming pool with 95000L of water with a pH of 8.9 needs to be lowered to a more suitable pH using an acidic substance. An ideal pH would be within the range of 7.2-7.6, so let's just assume that the pH we're hoping to achieve is 7.4. My brother chose...

Homework Statement A mixture is made by adding 25 ml of 0.100M HCl to 100ml of 0.025M ammonia hydroxide. Kd = 1.76 x 10^-5 . My task is to calculate the pH. Homework Equations I think this is the reaction that follows: NH4OH + HCl <--> NH4 + H2O + Cl The Attempt at a Solution I...

Homework Statement If .0200L of .100M nitrous acid is titrated using .200M NaOH solution, what will the pH be at equivalence? Homework Equations The Attempt at a Solution I figured out that the volume of NaOH at equivalence is .01L, however I do not know what to do after that...

Homework Statement Calculate the pH of a buffer made with 10.0 g of K2HPO4 and 5.0 g of KH2PO4 in 1.0L of water. Homework Equations -log Ka + log (base/acid) = pH The Attempt at a Solution So...mathwise, I know how to do this problem. My only question is, aren't K2HPO4 and KH2PO4...

how i find the pH of 5.525 gr HClO that melted in 100 ml solution? i just know i have 1 mol HClO, so how i keep from here? thanks.

which acid is more strong HNO3 or HBr? i get the the pH for HNO3 is 5 and for HBr is 2 is it Possible if HNO3 is more strong acid so it must have the low pH than HBr yes? thanks

i need to Calculate the pH of 1x10^-2 NaOH so i did like this: [OH-]=10^-2 POH=-log[OH-]=-log[10^-2]=2 and if i work with the Formula :pH+POH=14 so i will get pH+2=14 so the for the 1x10^-2 NaOH the ph=12 do i correct? thnaks.

A solution contains 0.200 mol HC2H3O2, 0.200 mol NaC2H3O2, and enough water to make 1.00 L of solution. a) Calculate the hydronium ion concentration. b) Calculate the new hydronium ion concentration after the solution is diluted to 2.00 L For a), I know the pH is just the same as the pKa of...

Homework Statement A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia and 1.00 moles of ammonium chloride in water to form a solution with a volume of 1.00L. To a 200 mL aliquot of this solution was added 10.0 mL of 10.0 M sodium hydroxide. What was the resulting pH...

Homework Statement Determine the pH when 0.39 mol HOCl is added to sufficient water to make 1.000 L of solution. (Ka (HOCl) = 3.700 x 10-8) Homework Equations Ka = Kw/Kb pH = -log(pKa) + log(acid/base) The Attempt at a Solution For this question first we need the concentration...

Homework Statement Homework Equations The Attempt at a Solution I have no idea how to solve this. Any info would be helpful.

what is the pH of a 0.140M NaOCN solution? ka HOCN=3.5x10^-4 (rule of 100 can simplify 0.140-x to 0.140) i know that ka=HOCN*OH^-/OCN^-=x^2/0.140 but i don't know the left hand side...i don't know what to do with HOCN=3.5x10^-4..

Homework Statement In our chemistry lab, we estimated the pH values of various solutions using six different indicators. Based on these estimated pH values, we must calculate [H+] and the estimated Ka or Kb values. Homework Equations For pH - ph=-log[H+} For Ka and Kb values -...

Homework Statement ka= 5.293 x 10^-6 using Ka, calculate the ph of a solution that contains equal concentrations of HB and B-. Homework Equations ph = -log[H+] The Attempt at a Solution im guessing that HB is the acid and B- is the base

I did an experiment and i AM A FIRST YEAR STUDENT AND I NEED HELP EXPLAINING WHAT TOOK PLACE. I ADDED 1% STARCH TO THREE TEST TUBES AND THEN 1 DROP IODINE. THEN IN ONE THE TUBE I ADDED 3 DROPS OF 1M NaCl AND then to another i added 3 drops 1M HCl and then i added to the last one i added 3 drops...

how to calculate the pH of a mixed solution containg 0.200M HA and 0.2 HB ka of HA =1.0^10-5 KA OF HB = 1.0^-6

I'm not looking for an indepth howto, I can look that up... I've only taken up to High School chemistry but I have intentions to research further into chemistry on my own before I get into university. Say I have a solution of a known quantity and known pH, and I want to add a currently...

Homework Statement Use the information below to answer the following question(s). methyl orange: red at pH < 3.1: orange at pH 3.1-4.4: yellow-orange above pH 4.4 litmus: red at pH < 4.5: purple at pH 4.5-8.3: blue above pH 8.3 thymol blue: yellow at pH < 8.0: green at pH 8.0-9.6...

pH INDICATORS...I DONT GET IT :( [b]1. Homework Statement Hello! I don't really need homework help...I'm actually studying for my final exam and I have a couple of sample questions that I have no idea how I would go about solving. What I would appreciate is if someone could explain to me...

[SIZE="3"]I'm not a chemistry student. So, I humbly request you to limit yourself to the basics, please do not indulge in infighting. If you ignore the request, you would be investing your efforts at the wrong place and perhaps it would be considered a pretentious show of knowledge. Litmus is...

Does anyone have a suggestion for learning about the pH of UO2SO4 in H2O?

Hello. This is probably a really dumb question, but I was wondering how the ph system works in relation to making a ph 7 liquid (which would be water and salt, right?) The way I was thinking was if you have an acid with a ph3 and a base with a ph8, and you wanted to mix them to produce a ph7...

Homework Statement Hi, I really don't get how to calculate the pH of a buffer solution...I mean I know that the pH of a solution is the negative log of the H3O+ concentration but I don't know how to get to that part...here's the problem...and I would appreciate if someone could actually...

The pH of our blood ranges normally from 7.35 to 7.45. My question is that how this pH is maintained in our blood. Are there any reactions that keeps our blood almost neutralized ? !

how to take a PH for solid like cake ...?

Hello, I am currently getting ready to start applying Ph. D. programs, but I am unsure whether I want to continue with physics or materials science (I will graduate with degrees in both physics and materials science). I am wondering whether career options will be better for a physicist or...

Hi I am interested in the change in the stability of the oxidation states of manganese with pH Mn is a stronger oxidising agent in acid than in base which would lead you to believe that the higher oxidation states of Mn are more stable in alkaline conditions. Does anyone have a reason...

Hey guys, so I have a project on the pH meter. Basically on what it is, what it's used for, how it works, and what principles does it run on. It is a group project but we can't seem to figure out some points and we've become very confused! Mainly, it's how it works. We researched and...

am really stuck on this problem, can't seem to get to the right answer Homework Statement How many mL of a 3.00 M HCO3- solution must be added to 200 mL of a 0.200 M CO32- solution to make a buffer with pH = 10.30? Answer. 13.96 mL Homework Equations pKa + log([base]/[acid])=pH HCO3(-) -->...

Homework Statement A solid acid is dissolved in enough water to make 200 mL of a solution. 40.0 mL of the solution is titrated to a phenolphtalein end point with an NaOH solution. The neutralized solution and the remainder of the acid solution are then mixed and the pH of the resulting...

Question: What is the pH of a solution made by mixing 0.30 mol NaOH, 0.25 mol Na2HPO4, and 0.20 mol H3PO4 with water and diluting to 1.00L? My work: So I found that the Ka value of H3PO4 is 7.5*10^-3 and the Ka value of HPO4 (found in Na2HPO4) is 4.2*10^-13. Because Ka of HPO4 is so small...

Homework Statement What is the pH of a saturated Zn(OH)2 solution? Ksp = 1.2 x 10^-17 Homework Equations Ksp = [Zn2+] [OH-]^2 Zn(OH)2 <----> Zn2+ + 2OH- pOH = -log [OH-] pH = 14- pOH The Attempt at a Solution Ksp = 1.2 x 10^-17 = [Zn2+] [OH-]^2 Zn(OH)2 <---->...

Here is a problem I was working on but I do not have a solutions manual because Its an old textbook. I would just like someone to look over my work. Homework Statement Calculate the pH of a 0.67 M NaClO solution. NaClO -> Na+ + ClO- ClO- + H2O -> HCLO + OH- Kw = 1.0*10^-14 Ka...

This isn't really homework, Its just a problem I'm trying to learn to solve. I'm not taking a chemistry course so I'm learning on my own. Calculate the pH of a solution that is 0.65 M NH4OH and 0.35 M NH4Cl. Well we can calulate the pOH = -log(OH-) and 14-pOH = pH I guess I need the...

Homework Statement Determine the pH of0.15 M solution of sodium acetate, ka = 1.8 x 10^-5 The Attempt at a Solution Since there are no hydrogen ions that dissolve from sodium acetate, would I use the pH of water =7.0? Is the pH of water even affected by sodium acetate?

for example, ethanoic acid in water, "="means equilibrium arrows CH3COOH(aq) + H2O(l) = CH3COO-(aq) + H3O(aq) we take the pH as the -log of the concentration of H3O ions. BUT why do we not take in account the effect of the ethanoate ion with water which produces OH-? CH3COO-(aq) +...

The problem is: Calculate the pH of a solution created by mixing 200.0 mL of .400 M acetic acid and 200.0 mL of 1.00 M sodium acetate. I got 2.02 for the pH, but according to other people in my class that's the wrong answer. Could someone explain how to do this? I used the Initial, Change...

I started this thread a while ago but never figured it out in the end can someone tell me if my idea of this is correct or not. Lets say I add 2 moles of a weak acid acetic acid to a liter of water (at STP). If I'm not mistaken the acetic acid will dissociate slightly depending on its...

Homework Statement I need to know how to do the following. If I have 1L of water with a pH of 7 and I add 1mL Vinegar with a pH of 2.4, what will the pH of the solution then be? I now need to get the pH of the solution back to 7 by adding ammonia which has a pH of 11.6. How much of that do I...