what is the ph of 10 molar hcl
HCl (aq.) -----------------> H+ (aq.) + Cl- (aq.)
[H+] = [HCl] = 10 M
We know that,
pH = - Log[H+]
pH = - Log(10)
pH = - 1
What is the pH of a 0.640 molar HCl solution?
To a sample of K3PO4 you add in 1.5 molar equivalents of HCl. 1a. What is the most likely pH (or pH range) of the resulting sample? 1b. What is the predominant molecular form of the phosphate molecule as a result of adding in the HCl?
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What would be the pH if 10 mL of 0.100 M HCL was added to 1000 mL of pure water?
Please help with this problem, Thanks!
*Extra Info given:
NaOH molar mass= 40.00g/mol
HCl molar mass= 34.46g/mol
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